A student is asked to determine the value of K, for hydrocyanic acid by titration with sodium hydroxide. The student begins titrating a 46.7 mL sample of a 0.449 M aqueous solution of hydrocyanic acid with a 0.255 M aqueous sodium hydroxide solution, but runs out of standardized base before reaching the equivalence point. The student's last observation is that when 50.0 milliliters of sodium hydroxide have been added, the pH is 9.555. What is K, for hydrocyanic acid based on the student's data?

The molar solubility of M2X5 is 6.44 x 10-9 M. Determine the solubility product constant for M2X5.

The molar solubility of zinc sulfide in a 0.117 M sodium sulfide solution is _____ M.

Calculate Q to determine whether or not a precipitate will form in a solution containing 0.043 M Ca(NO,), and 0.0055 M NaF. Step 1: identify the possible precipitate. In this example, it is Caf,. Look up its K value (table 16.2). Step 2: Write a balanced equation for dissolution of CaF,: Step 3: Write the equation for K, for CaFa: Step 4: Write an expression for Q: Step 5: Plug in the concentrations above to calculate Q: Step 6: Compare the value of Q to the value of K What will happen?

An aqueous solution contains 0.31 M ammonia.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added. More than one answer maybe required.) a) 0.32 mol HNO3 b) 0.31 mol Ba(NO3)2 c) 0.16 mol HNO3 d) 0.32 mol NH4NO3 e) 0.16 mol NaOH

The solubility product for chromium(III) fluoride is Ksp = 6.6 × 10⁻¹¹. What is the molar solubility of chromium(III) fluoride? A) 1.6 × 10 ⁻⁶ M B) 1.6 x 10⁻³ M C) 6.6 x 10⁻¹¹ M D) 2.2 x 10⁻³ M E) 1.3 x 10⁻³ M

ences to access important va An aqueous solution contains 0.33 M nitrous acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.17 mol HNO3 0.083 mol Ca(OH)2 0.34 mol HNO3 0.33 mol Nal 0.34 mol NaNO2

The molar solubility of iron(II) hydroxide in a 0.248 M iron(II) acetate solution is  M.

In a saturated aqueous solution of SrF,, the strontium ion concentration is 8.55 × 10–4 M and the fluoride ion concentration is 1.71 x 10-3 M. Calculate the solubility product, Ksp, for SrF,. Ksp

The molar solubility of nickel(II) carbonate in a 0.223 M sodium carbonate solution is ______ M.