Answer
D) Add 0.50mol KOH to the buffer
Explanation
A buffer solution is a combination of weak acid and its conjucate base or weak base and its conjucate acid
given buffer is combination of weak acid HCN and its conjucate base CN-
If NaOH is added to this buffer , as a base NaOH react with HCN
HCN + OH- ------> CN- + H2O
1:1 molar reaction
Initial mole of HCN = 0.15mol
Initial mole of CN- = 0.60 mol
moles of NaOH added = 0.50mol
0.15 moles of NaOH react with 0.15 moles of HCN to produce 0.15 moles of CN-
So, addion of NaOH destroy the buffer by removing the combination of HCN/CN-
A 1.0 L buffer solution has 0.15 mol L-'HCN and 0.60 mol L-1 KCN. The K,...
which one of the following is a buffer solution? a) 0.40 M HCN and 0.10 KCN b) 0.20 CH3COOH c) 1.0 M HNO3 and 1.0 NaNO3 d) 0.10 M KCN e) 0.50 M HCl and 0.10 NaCl
Questions 1: A) Calculate the pH of a buffer solution that is 0.246 M in HCN and 0.166 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). B) Calculate the pH of a buffer solution that is 0.200 M in HC2H3O2 and 0.160 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) C) Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of the...
5. If a buffer solution contains 0.0100 mol of KCN and 0.0100 mol HCN at pH = 8.50, what is the new pH after the addition of 5.00 x 10 mol HCI? The K for HCN is 6.2 x 10-10.
Which one of the following mixtures is a buffer solution? 0.40 M HCN and 0.10 KCN 0.20 M CH3COOH 1.0 M HNO3 and 1.0 M NaNO3 0.10 M KCN 0.50 M HCl and 0.10 NaCl
Part A. Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.171 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.230 M in HC2H3O2 and 0.170 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid NaOH.
Which of the following cannot be a buffer solution? Group of answer choices 1.0-L solution, in which 0.10 mol acetic acid (CH3COOH) and 0.050 mol potassium hydroxide (KOH) are dissolved. 0.50-L solution, in which 0.25 mol ammonia (NH3) and 0.18 mol hydrochloric acid (HCl) are dissolved. 0.75-L solution, in which 1.0 mol hydrofluoric acid (HF) and 2.0 mol sodium hydroxide (NaOH) are dissolved. 1.0-L solution, in which 3.0 mol lithium hydroxide (LiOH) and 5.0 mol formic acid (HCOOH) are dissolved....
A 1.0 L buffer mixture contains 0.15 moles of HClO and 0.20 moles of NaClO. Which of the following additions would destroy the buffer (exceeds the buffer capacity)? A. Adding 0.20 moles of NaOH B. Adding 0.15 moles of HCl C. Adding 0.20 moles of NaClO D. None of the above
A 1.0-L buffer solution initially contains 0.25 mol of NH3 (Kb=1.76×10−5) and 0.25 mol of NH4Cl. In order to adjust the buffer pH to 8.85, should you add NaOH or HCl to the buffer mixture? What mass of the correct reagent should you add?
34/35 A buffer solution is made that is 0.411 M in HClO and 0.411 M in Nacio. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.122 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made that is 0.365 M in HCN and 0.365...
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