Fill in the blanks: A buffer solution is consists of 0.100 M HCN and 0.200 M NaCN. HCN + H₂O <---> H30* + CN K₂ = 6.2 x 10-10 1. What is the pH of this solution? pH = 2. Calculate the pH if 0.025 M HCI is added to the solution. pH = 3. Calculate the pH 0.020 M NaOH is added to the solution (original). pH = Note: Type only your answer, expressed in 3 significant figures.

Fill in the blanks: A buffer solution is consists of 0.100 M HCN and 0.200 M NaCN. HCN + H₂O <---> H30* + CN K₂ = 6.2 x 10-10 1. What is the pH of this solution? pH = 2. Calculate the pH if 0.025 M HCI is added to the solution. pH = 3. Calculate the pH 0.020 M NaOH is added to the solution (original). pH = Note: Type only your answer, expressed in 3 significant figures.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What will the pH of 1.50 L of pure water water be if 2.0 mL of 4.0 M HCl is added? By how much has the pH changed? What will the pH of the solution in part b be if 2.0 mL of 4.0 M HCl is added? By how much has the pH changed? c. What will the pH of the buffer in part c be if 2.0 mL of 4.0 M HCl is added? By how much has the pH changed?
Given a solution in a volume of 200 ml of HCN 0.3M. We titrate the acid with a 0.75 M KOH solution. HCN Ka=4.9x10-10 1) Calculate the pH values after titration of the following amounts of the base. - 0 ml - 40ml - 80 mL - 100 mL
6. Calculate the pH of the resulting solution when 20.0 ml of 0.25 M HCl is added with 20.1 ml of 0,25 M NaOH ?
Consider a buffer solution comprised of HF and F. The K₂ of HF is 6.3 x 10-4. If the pH of the buffer solution is 2.96 and [HF] = 0.115 M, how many moles of F* are present? The volume of the buffer solution is 426 mL. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:
20. mL of 0.250 M NH3 is titrated with 0.500 M of HCl solution, what is the pH of the resulting solution when 0mL, 5.0 mL, 10.0 mL and 12 mL of HCl was added into the NH3solution? KB(NH3) = 1.8 x 10-5
A volume of 25.0 mL of 2.75 M HCl, is to be titrated with 1.025 M strong base, B(OH)2. Calculate the ff: A. pH of the resulting solution when the original solution has been titrated with 50.0 mL of the base titrant. B. pH of the resulting solution when the original solution has been titrated with 60.0 mL of the base titrant. C. pH of the resulting solution when the original solution has been titrated with 70.0 mL of the base titrant.
A 1.0-L buffer solution contains 0.100 mol acid, HA, and 0.100 mol base, NaA. The value of K, for the acid HA is 1.8x104. Ignoring the small volume change, what is the most likely pH of the solution if a 10.0 mL- sample of 1.00M HCI is added to the original buffer? O 1.20 < pH < 1.45 O 5.50 < pH < 5.74 O 4.10 < pH < 4.22 O 3.51 < pH < 3.69
I. Consider a 1.00 L of 1.50x10^-3 M hydrocyanic acid (HCN, K=4.9×10^-10) 1. Write the equilibrium expression. 2. Calculate the pH of the solution. 3. If a 9.00x10^-4 mol sodium cyanide, NaCN, is added, what is the pH of the resulting solution? Assume negligible volume change.
A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10. ( PREV 1 3 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp 3.8 x 10-10 %3D %3D 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5) [1.6 x 10-10] [3.8 х 1011 [x + 4.20] [x - 4.20] [x + 6.3 x 10-51 [x - 6.3 х 10-5] [x + 1.6 x 101°] [x - 1.6 x 10-10] [x + 3.8 x 10-101 [x - 3.8 x 101°]
Please answer all 3 questions
Consider a buffer solution contains 0.20 M NaF and 0.30 M HE:- (K, (HF) = 5.0 x 104 What is the pH of this solution? Choose.. Calculate the pH after 0.025 mol of NAOH is added to the buffer Choose... Calculate the pH after 0.02 mol of HCI is added to the buffer Choose...
Given two buffer solutions: Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO Buffer 2 : 2.00 M CH3COOH - 2.00 M NaCH3COO (Ka CH3COOH=1.8x10-5) In terms of pH, which is correct? i. Buffer 1 = Buffer 2 ii. Buffer 1 < Buffer 2 iii. Buffer 1 > Buffer 2