pH i got from previous question which was calculate the pH of a 1.00L buffer solution that is 0.100M in HF (Ka6.80*10^-4) and 0.150M in NaF. (not sure if needed but answer was 3.35pH). Please help with problem below.calculate the pH of the buffer after the addition of 10.0mL of 0.200M NaOH.

To calculate the pH of the buffer solution after the addition of NaOH, we need to consider the…

Answered: pH i got from previous question which…

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter25: Ph Measurements-buffers And Their Properties

Section: Chapter Questions

Problem 5ASA

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You have a weak acid concentration of 0.120 M and the conjugate base concentration is 0.100 M. What is the pH of this buffer? The Ka of this weak acid is 1.24x10-8 answer is 7.83, please explain how with steps
We have 500.0 mL of a buffer solution that is 0.684 M in NH3 and 0.339 M in NH4Cl. We add 500.0 mL of a solution 0.238 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution? Please type answer not write by hend
Chemistry need help with question 5 part B please 5. What amounts of reagents are needed to make the following buffer solutions? amchioride. B) 100.0 mL, pH = 8.85, lesser component = 0.10M, using 0.50 M HCN and 1.0 M NaCN.
If a buffer solution contains 2.1 M acetic acid and 2.7 M sodium acetate, what is the pH of the buffer if the K, of the acetic acid is 1.8 x 10-5. Round to 2 decimal places. Your Answer: Answer
A chemistry student is studying the effect of buffers. During his experiment, he collected the following data. However, is advisor informed him that his conclusions were incorrect. What are the likely conclusions the student provided that led to his advisor telling him this? (Select all that apply) Moles of pH of pH of buffer pH of buffer HCI water added (0.10 M HA/ (0.20 M HA/ Select 2 correct answer(s) 0.10 MA) 0.20 MA) O Buffer 2 is more concentrated, so its capacity to resist to changes in pH is higher than Buffer 1. 7.00 4.74 4.74 10-6 6.00 4.74 4.74 Any concentration of HCl will decrease the pH of water, while high concentrations of HCl is needed to change the pH of a buffer. 10-5 5.00 4.74 4.74 10-4 4.00 4.74 4.74 O Buffer 1 is less concentrated, so its capacity to resist changes in pH is higher than Buffer 2. 10-3 3.00 4.74 4.74 10-2 2.00 4.66 4.70 Adding HCl will increase the pH of water, but not the pH of the buffers 10-1 1.00 2.72 4.27
Please please please answer everything as fast as possible it is super important
A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka of acetic acid is 1.8 x 10-5. What is the pH of the solution if 0.11 mol of NaOH is added to 1.00 L of the solution? (Assume there is no volume change.) Round to 2 decimal places. Your Answer: Answer
2, In chemistry lab you make a buffer solution by dissolving 0.825 g of potassium formate in 0.2000L of 0.350 M formic acid. What is the initial pH of this buffer solution, and what is the pH after the addition of 10.50 mL of 0.235 M hydrochloric acid?
I dont know these two questions. Please answer both
Please get it right please ??
( Please type answer note write by hend )

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pH i got from previous question which was calculate the pH of a 1.00L buffer solution that is 0.100M in HF (Ka 6.80*10^-4) and 0.150M in NaF. (not sure if needed but answer was 3.35pH). Please help with problem below. calculate the pH of the buffer after the addition of 10.0mL of 0.200M NaOH.