Solve for the pH of a 0.0986 M solution of NaCN. Given
Ka (HCN)= 6.2 * 10-10
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Solve for the pH of a 0.0986 M solution of NaCN. Given Ka (HCN)= 6.2 * 10-10...
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
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
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A solution contains 0.50 M hydrocyanic acid (HCN; Ka = 6.2 × 10–10 at 25 °C) and 0.25 M sodium cyanide (NaCN) at 25 °C. Calculate the pH of this solution. Show (or explain) your calculation.
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 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
. ? 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