What is the pH of a 0.136 M aqueous solution of potassium fluoride, KF? (Ka for HF = 7.2×10-4)

What is the ph of a 0.0320 M solution of hydrocyanic acid HCN (Ka=4.9×10^-10)

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.

40) What is the pH of a 0.0140 M Ca(OH)2 solution?

What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.220 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 × 10⁻⁴)

1) What is the pH of a 0.926M solution of acetic acid (Ka=1.8x10^-5)?

Classify the basicity of magnesium hydroxide, Mg(OH)2, based on its reactivity in aqueous solution. Choose 1 answer: A B Weak base Strong base

Calculate the pH of a 0.10 M aqueous solution of Ba(OH)2

Why is the pH value for pure water 7 at 25 °C? What happens to the pH value for pure water if the temperature increases? Does it become more acidic or basic? Explain your answer. H2O (1) ⇒ H+ (aq) + OH- (aq)

What is the concentration of hydroxide ion in a 0.45 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 ✕ 10−14.) M What is the pH?