What is the pH of a 2.50 molar solution of NaCN(aq)? KA (HCN) = 6.2×10^-10
a. 11.80
b. 9.60
c. 9.21
d. 4.40
e. 2.20
A. is the correct answer
What is the pH of a 2.50 molar solution of NaCN(aq)? KA (HCN) = 6.2×10^-10 a....
Calculate the pH of a solution that is 1.50 M in HCN (Ka = 6.2 x10-10) and 0.50 M in NaCN. A. 3.44 B. 8.73 C. 9.68 D. 9.21 E. 3.63
8. The ionization constant, Ka, for HCN(aq) is 6.2 x 10". What is the pH of a 0.10 molar solution of sodium cyanide, which contains the cyanide ion? a. 5.10 b. 8.90 c. 9.21 d. 11.10 e. 11.30 9. The solubility product for Ag3PO, is: Kop = 2.8 x 101 What is the solubility of Ag,PO, in water, in moles per liter? a. 1.8 x 10M b. 2.5 x 10M c. 1.9 x 10 M d. 3.1 x 10M e....
Solve for the pH of a 0.0986 M solution of NaCN. Given Ka (HCN)= 6.2 * 10-10 Please have two decimal places for your answer.
Calculate the pH of a 0.75M aqueous solution of NaCN, Ka for HCN = 6.2E-10 Can someone explain to me how to do this problem step by step, and also explain why the reaction equation was written the way it was?? Calculate the pH of a 0.75 M aqueous solution of NaCN, K, for HCN is 6.2 X 1010. CNag)+ H2)HCNa)+ OH (aq) A/700 8) 9,21 15 0)479 A) 7.00 B) 9.2 C) 11.54D) 4.79 E) 2.46
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What is the pH of a 0.670 M solution of NaCN (Ka of HCN is 4.9x10^-10?
1. what is the pH of a .00300 M HCN solution? Ka of HCN is 6.2 x 10^-10 2. what is the pH of a .100 mL solution containing .50 M NaD and .20 M HF
Calculate the pH of a solution that contains 3.25 M HCN (Ka = 6.2 × 10–10), 1.00 M NaOH and 1.50 MNaCN. Question 14 options: A) 8.28 B) 7.46 C) 9.25 D) 8.86 E) none of these
What concentration of NaCN must be added to a 0.5 M HCN solution to produce a buffer solution with pH 7.0? Ka = 6.2 x 10–10 for HCN a) 3.3 M b) 0.49 M c) 6.9 x 10-5 M d) 0.0031 M e) 0.22 M
. ? Q1: Determine the pH solution contains 1.0 M of HCN (ka = 6.2 x 10-10) and HNO2 (ka = 4.0 x 10-4)? Correct answer is pH = 1.35