Question 20 3 pts What is the pH of a 1.0-L buffer solution composed of 0.025...
Question 22 3 pts What is the pH after 20.0 mL of 1.0 M HCl is added to a 1.0-L buffer solution composed of 0.75 M HCN and 0.15 M NaCN? 6.29 9.58 O 4.98 3.53 O 854
Question 3 10 pts 1.0 L of buffer solution is made from 0.17 mol citric acid and 0.11 mol sodium citrate. After adding 0.25 mol HCl to the buffer, what is the pH? Ignore the volume change. K, citric acid - 8.4e-4
QUESTION 3 What is the pH of a buffer solution composed of HA and A (Ka = 1.38 x 10-4) under these conditions: concentration of HA = 0.62, concentration of A = 0.65
What is the pH of the buffer solution in question 2 (Recall the values were: 1.0 L buffer of 0.35 M hydrofluoric acid (HF, Ka = 3.5x10-4) and 0.68 M sodium fluoride (NaF)) after 0.031 moles NaOH are added?
What is the pH of the buffer solution in question 2 (Recall the values were: 1.0 L buffer of 0.35 M hydrofluoric acid (HF, Ka = 3.5x10-4) and 0.68 M sodium fluoride (NaF)) after 0.052 moles of HCl are added? The answer is NOT 2.65
a. What's the pH after 10.0 mL of 0.10 M HCl is added to a 1.0-L buffer solution composed of 0.050 M HC3H5O3 and 0.025 M NaC3H5O3 b. Where in the titration process is a 30.0 mL of 0.10 M selenous acid, H2SeO3 with the addition of 22.5 mL of 0.20 M NaOH?
What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCl? 5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI?
1.What is the pH at which a buffer composed of NH3 and NH4+ would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15. 2. Consider a 1.0 L buffer containing 0.119 mol L-1 HF and 0.081 mol L-1 F-. What is the pH of the solution after adding 5.7 x 10-3 mol of NaOH? Express your answer to 2 decimal places....
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.45×10–8), and the conjugate base, A–, after 2.71 mL of 0.135 M HCl solution is added. The initial concentrations of the 142 mL buffer solution are [HA]=0.7 M and [A–]=0.37 M. Enter your value to two (2) decimal places.
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.58×10–5), and the conjugate base, A–, after 1.83 mL of 0.094 M HCl solution is added. The initial concentrations of the 133 mL buffer solution are [HA]=0.38 M and [A–]=0.67 M. Enter your value to two (2) decimal places.