converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.21 mol KCN

A solution is prepared by adding 150.0 mL of a 0.0100 M Mg(NO3)2 solution to 250.0 mL of a 0.100 M NaF solution. Will anything precipitate from this solution and, if so, what is the precipitate?   a. No, nothing will precipitate.   b. Yes, MgF 2   c. There is not enough information to answer this question.   d. Yes, Mg(NO 3 ) 2   e. Yes, NaNO 3

A solution contains 5.72×10-3 M potassium sulfate and 6.78×10-3 M ammonium fluoride.Solid lead nitrate is added slowly to this mixture.What is the concentration of sulfate ion when fluoride ion begins to precipitate?[sulfate] =  _______M

The solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp.       See Periodic Table If only 0.238 g of Ca(OH)2 dissolves in enough water to give 0.243 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?

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2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 M NaOH solution. a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1). Concentration (2) = 4.50 30.50mL b. Determine the molar mass of the acid. = 147.542 M=4-50 = 180 0.0025 3. Determine the K, for a monoprotic weak acid with a pH of 3.5 at half the equivalence point. Ka = 10-3.5 4. What color will the solution turn indicating that the equivalence point has been reached?

A solution contains 1.41×102 M chromium(III) nitrate and 5.91×103 M manganese(II) acetate. Solid potassium hydroxide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of hydroxide ion when this precipitation first begins? [OH] = M

16. Calculate the molar concentrations of all the cations and anions in a solution prepared by mixing 10.0 mL each of the following solutions: 0.100 M Mn(NO3)2, 0.100 M KNO3, and 0.100 M K2SO4

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A chemistry graduate student is given 250. mL of a 1.50M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 1º. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.84? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?