The concept used to solve this question is based on buffer solutions.
A Buffer solution is an aqueous solution of weak acid and it’s conjugated or vice versa. A buffer solution shows little change in pH when a small quantity of acid or an alkali is added to it.
Buffer are of two types acidic (buffer with pH<7) and basic (buffer with pH>7). The acidic buffer is made up by the combination of weak acid and conjugated base and on the other hand a basic buffer consists the combination of weak base and its conjugated acid.
A combination of weak acid and weak base cannot act as a buffer. A solution of weak base cannot act as a buffer. A solution of weak acid cannot act as a buffer.
Moreover, a strong acid and base pair can also not act as buffer as it would react and form a neutral salt.
Solution of weak acid HCN and its salt KCN can act as buffer. dimers in the solution so it cannot act as a buffer. and will form a neutral salt. KCN is a weak base. HCl and NaCl are strong acid-base pair they will form a neutral salt.
Ans:A solution of 0.40 M HCN and 0.10 M KCN will act as a buffer.
which one of the following is a buffer solution? a) 0.40 M HCN and 0.10 KCN...
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
A 1.0 L buffer solution has 0.15 mol L-'HCN and 0.60 mol L-1 KCN. The K, of HCN is 4.9 X 10-10. Which action will destroy the buffer? A. Add 0.50 mol HCN to the buffer. B. Add 0.50 mol KCN to the buffer. C. Add 0.50 mol HCl to the buffer. D. Add 0.50 mol KOH to the buffer. E. More than one of the above will destroy the buffer. (Hint: write some chemical equations & use stoichiometry!)
Which of the following solutions is a good buffer system? Question 8 Unanswered Which of the following solutions is a good buffer system? a solution that is 0.10 M HNO3and 0.10 M NaNO3 a solution that is 0.10 M LIOH and 0.10 M HNO3 a solution that is 0.10 M HCN and 0.10 M С LICN a solution that is 0.10 M HCN and 0.10 M NaBr a solution that is 0.10 M NaCl and 0.10 M HC E B...
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...
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...
Which one of the following is a buffer? a)A solution containing 0.10 M SrBr2 and 0.10 M HBr. b)A solution containing 0.10 M LiF and 0.10 M KF. c)A solution containing 0.10 M BaI2 and 0.10 M Ba(OH)2. d)A solution containing 0.10 M NaCN and 0.10 M HCN.
Which pair of compounds will form a buffer in aqueous solution? HCN and NaCN HCl and NaOH NaCN and NaOH HCN and HCl HCl and NaCl NaCN and KCN
A buffer solution is 0.392 M in HCN and 0.206 M in KCN. If K, for HCN is 4.0x1010, what is the pH of this buffer solution?
Which of the following could you add to 100.0 mL of 1.0 M HCN to make a suitable buffer system? (There may be more than one correct answer.) 100.0 mL of 0.050 M NaCN, 100.0 mL of 0.20 M NaCN, 100.0 mL of 1.0 M NaCN, 100.0 mL of 0.050 M NaCl, 100.0 mL of 0.20 M NaCl, 100.0 mL of 0.050 M HCN, 100.0 mL of 0.20 M HCN, 100.0 mL of 1.0 M HCN, 50.0 mL of 1.0...
Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L–1 aqueous HCN, will produce a buffer solution? 0.350 mol L –1 NaOH 0.10 mol L–1 CH3COOH 0.20 mol L –1 HCl 0.20 mol L–1 NaCN 0.10 mol L –1 HCl