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1. Calculate the pH of a 0.048 M solution of NaCH3COO. (Sodium acetate) [4]

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 61E: Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?

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1. Calculate the pH of a 0.048 M solution of NaCH3COO. (Sodium acetate) [4]

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Ff.5.
all one question :)
6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)
2. Explain the term 'buffer capacity'.
I just need help on questions 2 and 3.
Gg.174.
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, - log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L-' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kh for ammonia is 1.8 × 10–5. pKa base] pH = pKa +log acid Express your answer to two significant figures and include the appropriate units. Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. • View Available Hint(s) ? X•10n Value mass of NHẠCI = Units
A 1.00 liter solution contains 0.52 moles hypochlorous acid and 0.40 moles potassium hypochlorite. If 0.20 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) A. The number of moles of HC1O will decrease. ⒸB. The number of moles of C10¯ will remain the same. C. The equilibrium concentration of H3O+ will decrease. ⒸD. The pH will remain the same. [HCIO] [C10¯] ⒸE. The ratio of will increase.
G.37.
all one question :) thank you Part A: Calculate the pH of a buffer solution that contains 0.950 M CH3NH2 and 1.00 M CH3NH3Cl. (Kb = 4.4×10-4). pH of buffer = Part B: 20.0 mL of 1.00 M NaOH is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the NaOH(aq) is added? pH after NaOH added = Part C: 15 mL of 1.15 M HNO3 is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the HNO3 is added? pH after HNO3 added =
2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH3COOH with 9.00 mL of0.080 M NaOH.a. Calculate the moles of CH3COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH3COOH andCH3COOpresent in the buffer solution. c. Calculate the concentration of CH3COOH and CH3COOin the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffersolution. CH3COOH Ka = 1.8 x 10-5