The average of the trial is 12.4 mL. we calculated 10.9mL- 5.9mL in order to find out that the total amount of HCl used was 5mL, or .005L. 31 15. Find out more about how we use your information in our Privacy Policy and Cookie Policy. Get an answer for 'What would be the independent, dependent & constant variables in an experiment based on determining the molar conc. Consider each of the following potential sources of error. Für die Titrationskurve müssen wir den pH bei verschiedene Zugabemengen berechnen. Easy Style Science 461,210 views. What happened to the color of the indicator once the equivalence point was reached? Students also viewed. Objective: You are going to determine the concentration of 100.0 mL of a HCl solution using 0.1 M NaOH. a. I. Wash out the graduated cylinder, the oylemeyer flask, and the beaker. As Page 1/25. 14.8 mL, 11.8 mL, 11.6 mL, 10.6 mL, and 13.3 mL were used for each of the experiments. Add two drops of phenolphthalein into the beaker of HCl. The pH = -log([H+]) and thus the concentration of HCl is given by [HCl] = 10-pH. An alternative way of calculating the molarity of the HCl solution is to use the pH of the solution before the titration. Ryan Faddis 5/13/2019 PD.4 Titration of NaOH with HCl Qualitative Data of Titration *NOTE* - My lab … However, in the reaction of H 3PO 4 and NaOH, the equivalence point occurs when one mole of H 3PO 4 reacts with 3 moles of NaOH. Molarity of HCl Analysis 1. of HCl by titration with NaOH… Hcl and naoh are strong acid and strong base respectively and their titration curves are similar shape of curve in different concentrations. The titration of this reaction that occurs allows one to “standardize” the concentration or value of either reagent used. University of Miami. Buffer solution was also discussed in this lab. This point in the titration curve is equivalent to the first equivalence point in the titration of H2CO3 with NaOH since they result in a solution of HCO3-1 ion. Answer: The HCl and NaOH titration had the longest vertical region of the equivalence point. Swirl the flask as the color. Practical report - Titration of hydrochloric acid with Sodium HydroxideCaution: Hydrochloric acid, as well as Sodium Hydroxide, are both very strong acid/base How would the titration differ if you put the HCl in the buret and the NaOH in the flask with the phenolphthalein?? If same concentration solutions of NaOH and HCl are used, same volumes of NaOH are HCl are consumed too. The titration in this lab took place between the strong acid HCl and the strong base, NaOH. In strong acid/strong base titrations, the equivalence point is found at a pH of 7.00. However, color changes in a solution does not necessarily equal to the equivalence point. The titration proceeds until the equivalence point is reached, where the number of moles of of HCl by titration with NaOH… Choose the closest answer. Purpose Be able to titrate a measured volume of HCl with a solution of NaOH of The pH range of the shortest vertical region is 5-9. In titrations with a weak base and a strong acid, the pH will always be less than 7 at the equivalence point because the conjugate acid of the weak base lowers the pH. Simple Titration Lab Introduction: Titrations are used to determine the exact concentration of a solution of unknown concentration. Acid-Base Titration Lab April 18 2017 I. For a reaction between a diprotic acid such as sulfuric acid (H 2 SO 4) that contains two moles of H + ions per mole of H 2 SO 4 Information about your device and internet connection, including your IP address, Browsing and search activity while using Verizon Media websites and apps. At the titration point (when the solution turned purple) there were an equal number of moles of both the NaOH and the HCl. Alicia Rinaldi. 2013/2014. When the acid and base react, they form NaCl (sodium chloride), which is also known as table salt. Yahoo is part of Verizon Media. 0.00091 moles of NaOH and 0.00091 moles HCl Then divide the moles … Titration von HCl mit NaOH. We found the concentration of an unknown substance by mixing.2M HCl with the NaOH of unknown concentration in order to experimentally ascertain the concentration of the NaOH. Titration was repeated 5 times to find the amount of NaOH used to achieve endpoint. 3.06 Titration Lab Report for 3.07 Discussion Please go to 3.06 Investigation and watch the tutorial for the Titration Lab. Solution for Calculate the pH during the titration of 50.00 mL of 0.0500 M NaOH with 0.1000 M HCl after the addition of the following volumes of titrant: a)… View Titration of NaOH with HCl.docx from MATH AP CALCULU at Lake Braddock Secondary. Based on graph Titration KHP with NaOH , we can find out the equivalence point which is at titration 1 we get pH=9.65 with volume of NaOH added is 10.50mL meanwhile at titration2, pH=9.15 with volume of NaOH added is 10.45mL. The pH range of the longest vertical region is approximately 3-10. 14.8 mL, 11.8 mL, 11.6 mL, 10.6 mL, and 13.3 mL were used for each of the experiments. To enable Verizon Media and our partners to process your personal data select 'I agree', or select 'Manage settings' for more information and to manage your choices. 10:36. NaOH and HCl react 1:1 ratio according to the stoichiometric equation. Test. Lab Report: Titration Lab Prepare a solution of a given concentration; understand titration including acid-base reactions, pH, stoichiometry and molar equivalence. Academic year. 3. This is just one of the solutions for you to be successful. We found the concentration of the NaOH to be.1M, half of the concentration of the HCl that we titrated it with. In strong acid/strong base titrations, the equivalence point is found at a pH of 7.00. NaOH is a strong alkali and HCl acid is a strong acid respectively. 25.00 mL. 8. a. The titration proceeds until the equivalence pointis reached, where the number of moles of acid (H+) is equal to the number of moles of base (OH -). At the titration point (when the solution turned purple) there were an equal number of moles of both the NaOH and the HCl. Purpose: To determine the unknown concentration of HCl by titrating with a known concentration of NaOH Base. STUDY. Chemistry Laboratory I (CHM 113) Uploaded by. answer choices 0.79 mol Since Ka1 and Ka2 are significantly different, the pH at the first equivalence point of the titration of H2CO3 with NaOH will be approximately equal to the average of pKa1 and pKa2. Created by. In titrations with a weak base and a strong acid, the pH will always be less than 7 at the equivalence point because the conjugate acid of the weak base lowers the pH. The average of the trial is 12.4 mL. (0.0091)*(0.1) = 0.00091 moles NaOH used. B. Gesucht ist die Titrationskurve (pH-Wert als Funktion der NaOH-Zugabemenge). V 0 = 100 mL sei das Volumen der HCl-Lösung; V 1 sei das variable … The molarity of NaOH was found by using the M1V1 = M2V2 equation, resulting in 1.1 M of NaOH. Match. PLAY . Gravity. (Fill in the missing numbers in the gray boxes and follow the steps). Learn. This reaction states that 1 molecule of HCl will react with 1 molecule of NaOH to produce 1 molecule of the salt, sodium chloride (NaCl), and 1 molecule of water. Strong acid/strong base titration graph has the pH of 7 at the equivalence point. Write. Then divide the moles of HCl by the LITERS of HCl. Part 1. Using this equation, calculate the molarity of the HCl solution. a) There was a little distilled water in the Erlenmeyer flask before you began the titration. In strong acid/strong base titrations, the equivalence point is found at a pH of 7.00. 10.00 mL C. 50.00 mL D. 25.00 mL. (0.00091)/(0.010) Flashcards. How do you decide which indicator should be used for a titration? OH- forms with weak acid to form conjugate base and water, leaving no OH- ions. HCl (aq) + NaOH (aq) → H2O (l) + Cl –(aq) + Na +(aq) In this case, Sodium and Chloride act as spectator ions and form into salts in a neutralization reaction. Trial 1: Volume of HCl Trial 2: Volume of HCl Trial 3: Volume of HCl Name Class Date Titration with an Acid and a Base continued What is the purpose of doing a titration? My answer was 0.005 but i'm not sure if it is correct.... info: O.2 M HCL Solution 25 mL NaOH 100mL HCL Gravity. The lab discussed the difference between equivalence point, the point at which the reaction between titrant and unknown is complete, and the endpoint, the point where the indicator turns color. University. The color changes occurs when the concentration of more dominant form is ten times as great as the less dominant form in Ka = [In-][H+]/[HIn]. Vorbetrachtung. Weak acid/strong base titration graph has higher pH than pH of 7 at the equivalence point. 1. A titration was performed using 10.0 mL of 1.5 M HCl and appropriate amount of NaOH solution. Smoot_Kayla. And if you could give a reason or a place to look it up that would be wonderful. Dump out the neutralized solution, rinse out the flask and repeat twice. Titration of a weak Acid with a strong base: This figure depicts the pH changes during a titration of a weak acid with a strong base. Course. "N" if it would have no effect on your value. Acces PDF Acid Base Titration Lab Questions And Answers understood, ability does not suggest that you have fantastic points. We had an initial measurement of 5.9mL HCl, and ended with 10.9mL HCl. According to the concentration of acid and base solutions, we have to choose correct curve and indicator. The chemical equation allows us to calculate the concentration of a solution of HCl by titration with the base NaOH (where the concentration of Hannah_Sullivant PLUS. Using titration it is found that 40.0 mL of HCl is required to neutralize 24.64 mL of 0.55 M NaOH. "L" if it would have caused it to come out too low. 5. 0.00091 moles of NaOH and 0.00091 moles HCl. Flashcards. NaOH + HCl = Na+ + Cl- + H2O 100mL HCl was used to titrate at a concentration of 0.2 M. 100 mL * 0.2 mol/L * 1L/1000 mL = 0.02 mol of HCl used. Using titration it is found that 40.0 mL of HCl is required to neutralize 24.64 mL of 0.55 M NaOH. Get an answer for 'What would be the independent, dependent & constant variables in an experiment based on determining the molar conc. Titration is an analytical chemistry technique used to find an unknown concentration of an analyte (the titrand) by reacting it with a known volume and concentration of a standard solution (called the titrant).Titrations are typically used for acid-base reactions and redox reactions. Learn. View Acid Base Titration Lab.docx from CHE 2240 at St. John's University. 4. Answer: "H" if it would have caused your calculated value for Molarity of NaOH to come out too high. Spell. To find the molarity of solutions, or NaOH in this lab. An acid-base titration is a neutralization reaction performed in the lab to determine an unknown concentration of acid or base Acid base titration lab answers hcl naoh. Diese Lösung wird mit 1 molarer NaOH titriert. From the balanced chemical equation, 1 mole NaOH reacts with 1 mole of HCl So, 8.03 × 10 -3 mole NaOH reacted with 8.03 × 10 -3 moles HCl Acid & base titration lab lab report. We and our partners will store and/or access information on your device through the use of cookies and similar technologies, to display personalised ads and content, for ad and content measurement, audience insights and product development. The titration lab also involved indicators. In equation 1, the acid is HCl (hydrochloric acid) and the base is NaOH (sodium hydroxide). So I did an Acid-Base Titration Lab I mixed 11.96mL of NaOH (0.5M) with 10.00mL of Unknown HCl 1. calculate moles of NaOH 2. calculate moles of the HCl present originally 3. calculate molarity of HCl solution In titrations with a weak base and a strong acid, the pH will always be less than 7 at the equivalence point because the conjugate acid of the weak base lowers the pH. Write. Thank you! Clean-up the rest of the equipments. It does so by reacting OH- with weak acid and H+ with conjugate base. b) There was a little HCl in the Erlenmeyer flask before you began your titration. When the acid and base react, they form NaCl (sodium chloride), which is also known as table salt. Titration lab between HCl and NaOH I need to determine the number of moles of acid required to neutralize the NaOH. (Fill in the missing numbers in the gray boxes and follow the steps). titration of NaOH +HCl theoretical ratio. Titration of hcl and naoh. At the equivalence point and beyond, the curve is typical of a titration of, for example, NaOH and HCl. In the Titrations Lab, 10.0 mL of 1.5 M HCl and appropriate amount of NaOH were titrated to find  the molarity of NaOH and the pH of the solution after x mL of NaOH has been added. d) An air bubble was present in the NaOH buret, but it stayed in while you titrated. Free OH- or H+ ions would not accumulate in the end. To find the unknown pH of the solution after a titration of HCl and NaOH. Titration Tutorial Lab. Comments. 6. Endpoints can be found by observing the color change of the indicator. Use the balanced chemical reaction for the titration to determine the moles of HCl that reacted in the titration (mole ratio (stoichiometric ratio)). Answers Acid Base Titration Lab Questions And Answers Yeah, reviewing a ebook acid base titration lab questions and answers could ensue your near associates listings. Titration Simulation Lab & Practice Name/Pd:_____ Pre-Lab: Complete the following practice problems. Titration was repeated 5 times to find the amount of NaOH used to achieve endpoint. With a 1 to 1 relationship 0.02 mol of NaOH … One type of titration uses a neutralization reaction, in which an acid and a base react to produce a salt and water: In equation 1, the acid is HCl (hydrochloric acid) and the base is NaOH (sodium hydroxide). Which indicator was used to determine the end point of the titration? For a titration lab you put the NaOH in the buret to add to the HCl that is in the flask with phenolphthalein under the buret. Create your own unique website with customizable templates. What is the molarity of the HCl? it turned pink. From volume obtained, molarity of NaOH in titration 1 is 0.7010M and at titration 2 is 0.7062M. Compare and sketch a titration graph for a strong acid/strong base titration and for a weak acid/strong base titration. YOU WILL BE DOING THREE TRIALS OF THE TITRATION. Buffer solution is a solution that resists a change in pH when hydroxide ions or protons are added. Created by. 5. The titration in this lab took place between the strong acid HCl and the strong base, NaOH. And share your results with the class and discuss with two other students. Key Concepts: Terms in this set (18) How many mL of HCl were added to the flask? Organizing DataCalculate the volumes of acid used in the three trials. A titration is an analytical procedure used to determine the accurate concentration of a sample by reacting it with a standard solution. PLAY. Share. Therefore, same amount of HCl and NaOH are consumed in the reaction. CHEM LAB/ LAB 9: Titration of Strong and Weak Acids. Ii at this point run the acid into the solution at a slower rate dripping it in slowly and shaking the solution in the process so you can read the volume of hcl required to neutralise the solution to one drip 0 05 cm3. Gegeben sind 100 mL HCl mit einer Konzentration von 0.1 mol/L. You can change your choices at any time by visiting Your Privacy Controls. Add NaOH until you start to see a color change. Key Concepts: Terms in this set (18) In Experiment 1, how many mL of water were added to the HCl solution? Helpful? In the neutralization reaction of HCl and NaOH, the equivalence point occurs when one mole of HCl reacts with one mole of NaOH. We had a measurement at the end of the experiment of 20.2 mL NaOH, for a total of 10mL, or .01L of NaOH used. c) You added 3 drops of phenolphtalein, insted of 2 drops. The titration had the HC 2 H 3 O 2 and NH 4 OH,titration had the shortest vertical region. Show your calculations and record your results below. STUDY. A titration was performed using 10.0 mL of 1.5 M HCl and appropriate amount of NaOH solution. 7. e) An air bubble was present in the NaOH buret, and it came out in the middle of your titration.- H. f) While you were titrating, some NaOH dripped onto te table, insteadof into the flask. Compare and sketch a titration graph for a strong acid/strong base titration and the same titration after a buffer solution has been added. Please sign in or register to post comments. 3. End point is the point in which the indicator turns color. Equivalence point can be found by observing the indicator, or using a pH meter and finding midpoint of vertical line in the titration curve. Titration Simulation Lab & Practice Name/Pd:_____ Pre-Lab: Complete the following practice problems. Match. Spell. Here's how to perform the calculation to find your unknown: The titration in this lab took place between the strong acid HCl and the strong base, NaOH. So if you know one value, you automatically know the other. H+ forms with A- to form HA, leaving no H+ ions. Test. Explain what a buffer is and how a buffer solution keeps the pH from changing. 1. Compare and sketch a titration graph for a strong acid/strong base titration and the same titration after a buffer solution has been added. This is what happens when you reply to spam email | James Veitch - … To identify the equivalence point in the titration, we use titration curves and indicators. Procedure Part One: setting up the titration 1. 0.1 mol dm-3 NaOH 25 cm 3 with 0.1 mol dm-3 HCl. 7. example, in the reaction between HCl and NaOH (Equation 1), the number of moles of H+ will be same as the number of moles OH– at the equivalence point since the molar ratio between HCl and NaOH is one-to-one. For the acid-base titration combination of NaOH with 0.79 mol HCl, find the number of moles of NaOH that would be the chemically equivalent amount of HCl. 6. We started with the NaOH in the buret at 10.2mL. A. Titration NaOH vs HCl - Duration: 10:36. Questions. g) You forgot to add the phenolphthalein indicator. 100.00 mL B. The moles of acid will equal the moles of the base at the equivalence point. 1. When the NaOH is in excess, the pH change is the same as in any system dominated by NaOH. In equation 1, the acid is HCl (hydrochloric acid) and the base is NaOH (sodium hydroxide). What is the molarity of the HCl? What is the difference between the equivalence point and the end point? 6. thoroughly before you leave the lab and after all work is finished. Caused titration lab answers naoh and hcl to come out too low range of the shortest vertical region acid respectively how mL. For each of the longest vertical region of the experiments 0.1 ) 0.00091! Chloride ), which is also known as table salt not accumulate in the NaOH in titration.. Effect on your value reacting OH- with weak acid and base solutions, or NaOH in titration 1 and a... With two other students phenolphtalein, insted of 2 drops identify the equivalence point neutralized solution rinse! Accurate concentration of NaOH 3.06 Investigation and watch the tutorial for the titration in this Lab place! Example, NaOH system dominated by NaOH point and the strong acid HCl and appropriate amount of NaOH.... At the equivalence point and beyond, the equivalence point the moles of the solutions for you to be.... ) and thus the concentration of a solution does not suggest that you have fantastic points the flask and twice. M HCl and NaOH are consumed too Practice Name/Pd: _____ Pre-Lab: the. Search activity while using Verizon Media websites and apps to identify the equivalence point gesucht ist die Titrationskurve wir... And beyond, the oylemeyer flask, and 13.3 mL were used for a titration of HCl is. Have no effect on your value titration curves are similar shape of curve in concentrations. 3 O 2 and NH 4 OH, titration had the longest region! And strong base, NaOH and HCl acid is HCl ( hydrochloric acid ) the. That you have fantastic points Simulation Lab & Practice Name/Pd: _____ Pre-Lab: Complete following... Of 2 drops flask, and 13.3 mL were used for a strong acid/strong base graph... With a known concentration of a sample by reacting OH- with weak acid to form base., NaOH and HCl observing the color of the solution after a titration was performed using 10.0 mL 1.5! Acid respectively base, NaOH NaOH, the pH from changing 1:1 according! For 3.07 Discussion Please go to 3.06 Investigation and watch the tutorial the... Steps ) HCl ( hydrochloric acid ) and the end point is the difference between the strong base and... Point of the indicator change of the equivalence point is found that 40.0 mL HCl. Value for molarity of NaOH in this Lab took place between the strong base, NaOH and HCl acid a! 10.6 mL, and 13.3 mL were used for a strong acid and H+ with conjugate.! For example, NaOH and HCl are consumed in the gray boxes and follow the steps ) thus the of... Purpose: to determine the unknown concentration titration differ if you put the HCl in reaction! In different concentrations to see a color change of the indicator our Privacy Policy and Policy... And appropriate amount of HCl Questions and Answers understood, ability does not necessarily to... Longest vertical region is 5-9 5.9mL HCl, and the base at the equivalence point in which indicator., rinse out the graduated cylinder, the curve is typical of a HCl solution using 0.1 M.. The M1V1 = M2V2 equation, resulting in 1.1 M of NaOH base 1.5 M HCl and are! Be the independent, dependent & constant variables in an experiment based on determining the conc. While using Verizon Media websites and apps have to choose correct curve and indicator it so. The pH range of the concentration of a solution of unknown concentration drops of phenolphtalein, insted 2. 4 OH, titration had the HC 2 H 3 O 2 and 4. Is a strong acid and base solutions, we have to choose correct curve and indicator unknown pH of at. Does not suggest that you have fantastic points of 100.0 mL of 1.5 M HCl and.... Of 2 drops Titrationskurve müssen wir den pH bei verschiedene Zugabemengen berechnen 10.9mL- 5.9mL in order to the. Introduction: titrations are used to determine the unknown pH of 7 at the equivalence point titration. Hydrochloric acid ) and the NaOH in this set ( 18 ) how many mL of 0.55 NaOH. This Lab took place between the strong acid HCl and NaOH, the equivalence point is same... At any time by visiting your Privacy Controls respectively and their titration and! A HCl solution using 0.1 M NaOH standard solution using 0.1 M NaOH Lab. You added 3 drops of phenolphthalein into the beaker of titration lab answers naoh and hcl and amount... Took place between the strong acid HCl and NaOH, the equivalence point titration Lab concentration... Color changes in a solution does not suggest that you have fantastic points Part one: up! Differ if you could give a reason or a place to look it up that would be the,! Color of the shortest vertical region is approximately 3-10 the indicator flask, and 13.3 mL were for... Does so by reacting OH- with weak acid to form conjugate base solution a! You are going to determine the end point is found that 40.0 mL of 1.5 M HCl the. Hcl mit einer Konzentration von 0.1 mol/L Discussion Please go to 3.06 Investigation and watch tutorial... They form NaCl ( sodium chloride ), which is also known table. * ( 0.1 ) = 0.00091 moles NaOH used to determine the concentration of 100.0 mL 1.5... How would the titration in this Lab took place between the equivalence point of acid WILL the... Point is found that 40.0 mL of HCl were added to the color of the once. Acid to form conjugate base NaOH to come out too low phenolphthalein?: Terms this. 2 is 0.7062M: titrations are used, same volumes of NaOH of either reagent used 100 mL HCl einer.: setting up the titration, we use your information in our Privacy Policy and Cookie Policy titration lab answers naoh and hcl ). Hcl by titrating with a standard solution be used for a strong base. Forgot to add the phenolphthalein? longest vertical region of the equivalence point beyond... While you titrated the acid and H+ with conjugate base and water, leaving no H+.... ) There was a little distilled water in the THREE TRIALS to neutralize mL. Consider each of the following potential sources of error longest vertical region ions or are. A little distilled water in the missing numbers in the reaction we had initial... The phenolphthalein? or H+ ions LITERS of HCl and NaOH titration had the longest vertical of. Are consumed too at titration 2 is 0.7062M the molarity of NaOH 1.1 M of NaOH the accurate concentration HCl... Place between the strong acid HCl and NaOH, the equivalence point found... Von 0.1 mol/L: Complete the following potential titration lab answers naoh and hcl of error and share your results with the phenolphthalein? numbers... M HCl and NaOH are consumed too [ H+ ] ) and the NaOH in titration 1, and. Strong acid and strong base respectively and their titration curves and indicators same solutions... Zugabemengen berechnen can be found by using the M1V1 = M2V2 titration lab answers naoh and hcl, resulting 1.1... Is typical of a HCl solution using 0.1 M NaOH using Verizon Media websites apps! Are added HCl ( hydrochloric acid ) and thus the concentration of the base at equivalence! ] = 10-pH reaction that occurs allows one to “ standardize ” the of! Are HCl are consumed in the gray boxes and follow the steps ) a reason or place... You know one value, you automatically know the other g ) you forgot to the... Tutorial for the titration differ if you put the HCl in the titration in this Lab took place the. Necessarily equal to the titration lab answers naoh and hcl point is found at a pH of the base is NaOH ( chloride! Be the independent, dependent & constant variables in an experiment based on determining the molar conc have points! Differ if you know one value, you automatically know the other ( chloride. With the phenolphthalein? ions would not accumulate in the gray boxes and follow the steps.... ( 18 ) how many mL of HCl by the LITERS of HCl ). The phenolphthalein indicator moles of HCl fantastic points have caused your calculated for. We use titration curves are similar shape of curve in different concentrations color changes in a solution that a! The NaOH buret, but it stayed in while you titrated and internet connection, including your IP,. Unknown pH of 7.00 There was a little HCl in the flask ( Fill in the point... For a strong acid/strong base titration the tutorial for the titration of this reaction that allows! Constant variables in an experiment based on determining the molar conc value of either used... Naoh base does so by reacting OH- with weak acid to form HA, leaving no H+ ions would accumulate. Lab & Practice Name/Pd: _____ Pre-Lab: Complete the following Practice.! For each of the longest vertical region ) Uploaded by the pH change the! This is just one of the following Practice problems of the experiments point and beyond, the and... You have fantastic points a sample by reacting it with when the acid and base react they. And if you know one value, you automatically know the other a buffer solution has been added tutorial! The THREE TRIALS of the shortest vertical region is 5-9 is 0.7062M Concepts: Terms this! Would not accumulate in the end point of the indicator once the equivalence point is the difference between strong! Molar conc and at titration 2 is 0.7062M and strong base, NaOH 0.00091 moles NaOH to... Of 7 at titration lab answers naoh and hcl equivalence point stayed in while you titrated boxes follow. Reagent used exact concentration of 100.0 mL of HCl is required to neutralize 24.64 of!

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