Final buret reading after HCl addition, ml: 135 ml Volume of hydrochloric acid used, ml: 75 ml [OH-] in saturated Ca(OH)2 solution, M: ________ Calculated solubility product from titration: ________
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- Molarity of hydrochloric acid, M: .02
- Initial buret reading before HCl addition, ml: 0
- Final buret reading after HCl addition, ml: 135 ml
- Volume of hydrochloric acid used, ml: 75 ml
- [OH-] in saturated Ca(OH)2 solution, M: ________
- Calculated solubility product from titration: ________
- . Average value of solubility product from titration: _________
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- Please help me fill out this table! Answering just one of the columns is good enough, thank you! Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration _?_mmol _____mmol Millimoles of acetic acid in sample _?_mmol ______mmol Molar concentration of acetic acid solution _?_mol/L ______mol/LIn lab, you will be provided with a 1.8 M acetic acid solution (CH3COOH) and solid sodium acetate trihydrate (NaOOCCH3 3H2O). You want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. How many grams of sodium acetate trihydrate, and what volume (mL) of the 1.8M acetic acid solution and deionized water should you combine? The pKa of acetic acid is 4.75. Show all work.A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
- Propanoic acid that, along with its sodium salt, can be used to make a buffer that has a pH of 5.25. If you have 512.5 mL of a 0.272 M solution of that acid, how many grams of the corresponding sodium salt do you have to dissolve to obtain the desired pH? For propanoic acid, HC3H5O2, Ka = 1.3 x 10-5. m(salt) = Want solution ASAPI need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)Table 1: Qualitative Analysis of Group II Cations Group II Cations Confirmatory Reagent Result/ Observation Substance Formed Inference Write the chemical equations involve in the analysis of group II cations. Guide Question: What are differences of the precipitates of each cation in group II? Reference video : https://www.youtube.com/watch?v=BZGZZx1lHKA
- Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?PLEASE ANSWER ALL PARTS THANK YOU Given:Kb for ammonia of 1.8 X 10-5 Volume of NH3 in flask (mL): 10.00 Average Volume of HCl it took to get to equivalence point (mL): 20.50 Concentration of HCl (M): 0.100Volume of HCl added to calculate “beyond equivalence pH”(mL): 10.50 a) Calculate the concentration of the ammonia.b) Calculate the pH of the contents of the flask (NH3) before the titration begins.c) Calculate the pH of the contents of the flask in the titration at ¼ way to equivalence. This means use your volume added to get to eq point (mL) value but multiply it by ¼ (so you are not yet at equivalence).d) Calculate the pH of the contents of the flask in the titration at ½ way to equivalence (so also not yet at equivalence)e) Calculate the pH of the contents of the flask in the titration at the equivalence point.f) Calculate the pH of the contents of the flask in the titration beyond the equivalence point. Use your given amountThis is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
- calculations for acetate buffer solutions 1. moles of sodium acetate in in 250.0 mL acetate buffer (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Please present complete solution. Express your final answers up to two (2) decimal places.A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated