Calculate the mass (g) of potassium nitrate KNO_3 that is required to prepare 10

Question

Calculate the mass (g) of potassium nitrate KNO_3 that is required to prepare 100.0 mL of 0.10 M KNO_3(aq). The solubility product constant for Mg(OH)_2(s) is 1.2 Times 10^-11. Calculate the s magnesium hydroxide in mol/L and in g/L. The concentration of Pb^2+ ions and of CO_3^2- ions in a saturated aqueous solution of PbCO_3 is 1.8 Times 10^-7 M. Determine K_sp of PbCO_3. Calculate its solubility in g/L and in g/100 mL. Determine the molar solubility of AgCl in (a) pure water and (b) 0.10 M NaCl(aq). The K_sp of AgCl is 1.8 Times 10^-10.

Explanation / Answer

1 no of moles of KNO3 = Molarity * volume in L

                                   = 0.1* 0.1 = 0.01 moles

mass of KNO3          = no of moles * gram molar mass

                                = 0.01*101 = 1.01 g

2. Mg (OH)2 ------> Mg+2 + 2OH-

                                s          2s

Ksp   = [Mg+2][OH-]2

1.2*10-11 = s*(2s)2

1.2*10-11   = 4s3

3*10-12   = s3

   s         = 1.44*10-4 M

solubility of Mg(OH)2 1s 1.44*10-4 M   = 1.44*10-4 mole/L  

solubility of Mg(OH)2 1s                      = 1.44*10-4 mole/L   * 58g/mole

                                                              = 8.352*10-3 g/mole

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