Calculate the pH and equilibrium concentrations of a 0.46M salt solution of sodium cyanide NaCN in water. Write the balanced chemical reaction(s) and show your work. Ka(HCN) = 4.0x10-10. For the concentrations, input only the numeric answer.
What is the pH?
What is the HCN concentration?
What is the CN- concentration?
What is the OH- concentration?
What are the units of concentration?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Calculate the pH and equilibrium concentrations of a 0.46M salt solution of sodium cyanide NaCN in...
Consider a 0.375 M aqueous solution of sodium cyanide (NaCN). A) Write the reaction of the cyanide anion (CN-) with water. B) Calculate [OH-], pOH, pH. Also, calculate percent ionization. (Obeys 5% rule). (Ka of HCN = 4.9 x 10^-10)
Consider a 0.20 M solution of the salt, sodium cyanide, NaCN. A) What acid and What base reacted to from this salt? B) Classify the acid above as a strong or weal acid. Classify the base as a strong or weak base? C) Will the salt solution be acidic, basic, or neutural? D) Calculate the ph of the solution? The Ka of HCN is 4.9 x 10-10?
1) Cyanide salts such as Sodium Cyanide (NaCN) are among the most rapidly acting of all known poisons and act by inhibiting respiration. a. Determine the pH of a solution of 0.054M Sodium Cyanide (NaCN) (assuming complete dissociation) and state whether sodium cyanide is an acidic basic or neutral salt (Ka HCN = 4.9x10-9) (6 marks) Chemistry Class
REterencES Calculate the OH concentration and pH of a 1.8 x 10 M aqueous solution of sodium cyanide, NaCN. Finally, calculate the CN concentration. (Ka(HCN)= 4.9 x 10-10) M [Hol pH [CN )-
Calculate pH of a salt solution. What is the pH of a 0.172 M aqueous solution of sodium cyanide, NaCN? (K for HCN = 4.0x1010) pH
The pH of an aqueous solution of 0.210 M sodium cyanide, NaCN (aq), is This solution is
4. Calculate the pH of an 8.27 x 10-3M solution of sodium cyanide, NaCN.
A buffer solution contains 0.58 mol of hydrocyanic acid (HCN) and 0.68 mol of sodium cyanide (NaCN) in 3.00 L. The Ka of hydrocyanic acid (HCN) is Ka = 4.9e-10. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.46 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.23 mol of HI? (assume...
A 500.0 mL solution of NaCN was prepared from a 12.0g sample. What is the pH of the solution? (Ka for HCN is 4.0x10^-10)
Calculate the pH of a solution that is prepared by dissolving 0.470 mol of hydrocyanic acid (HCN, Ka = 6.17×10-10) and 0.180 mol of nitrous acid (HNO2, Ka = 4.60×10-4) in water and diluting to 2.30 L. Also, calculate the equilibrium concentrations of HCN, CN-, HNO2, and NO2-. Do not make an approximation unless the initial acid concentration is greater than 1000 × Ka. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCN]...