Calculate the OH concentration and pH of a 3.6 x 10-³ M aqueous solution of sodium cyanide, NaCN, Finally, calculate the CN concentration. (K. (HCN) = 4.9 × 10-10) [OH-] = M pH = [CN] = M

If the K of a weak base is 2.5 × 10-6, what is the pH of a 0.23 M solution of this base? pH =

Determine the |H*, pH, and pOH of a solution with an OH- of 8.5 x 10-13 M at 25 °C. [H*] = M pH = РОН

Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic pOH = 8.58 [H*] =3.4 x 10-2 pH = 8.24 [H+] = 5.4 x 10-12 pOH = 7.00 pH = 3.13 Basic Answer Bank [OH-] = 3.9 × 10-5 [OH-] = 1.3 x 10 Neutral [H]=1.0 x 10-7 pOH = 5.25

Part C Consider hydrocyanic acid, HCN, which is a weak acid. Which expression represents the K, of the conjugate base, CN ? HCN] O K, = |CN [H,O*] (CN] HCN||OH K, = [HCN||OH-] O K, (CN O K, = |CN-||H3O*] [HCN]

The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁴. What is [OH⁻]?   What is the concentration in %m/v of a 0.549 M aqueous solution of methanol (MM = 32.04 g/mol)?   The pH of a solution is 3.30. What is the OH⁻ concentration in the solution?

For the diprotic weak acid H2A, Kal = 3.0 × 10-6 and Ka2 = 7.1 x 10-9. What is the pH of a 0.0700 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A?- in this solution? [H,A] = M [A?-] = M

Many salts have basic properties because their anion can accept a proton from water. One example is sodium fluoride, sometimes used in toothpaste. F-(aq) + H2O(l) ⇌ HF(aq) + OH-(aq)                                                                                                                                       Find the concentration of hydroxide ions in an 0.07 mol/L aqueous solution, something close to what one could find in a typical toothpaste.[1] The fluoride ion’s Kb is 2.9 × 10-11. Show your work. An IRE or IREC table is not required but recommended. Justify any approximation you may make. What are the pOH and pH of the solution described in (a) (to 1 decimal figures)? You may assume a temperature of 25 °C. Show your work. If you were unable to solve (a), do your calculation with 0.00330 mol/L hydroxide ions.

Ammonia, NH3, acts as an Arrhenius base, a Brønsted-Lowrybase, and a Lewis base, in aqueous solution. Write out thereaction NH3 undergoes with water and explain what propertiesof ammonia correspond to each of the three definitionsof “base.”

What is the pH of an aqueous solution with [H3O+] = 2×10−14 M? Express the pH numerically using one decimal place.