Excess solid Na₂CO₃ is added to a solution containing 0.450 M (each) Mg²⁺ and Zn²⁺ ions. Ksp for MgCO₃ is 3.50 × 10⁻⁸ and Ksp for ZnCO₃ is 1.00 × 10⁻¹⁰. ZnCO₃, with the smaller Ksp, will be the least soluble and will begin precipitating first. What will be the [Zn²⁺] concentration when MgCO₃ just begins to precipitate? (Assume no volume change upon addition of the solid Na₂CO₃).

What you expect to observe on mixing 0.1M CuSO4 with 0.1M Na2CO3. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?

A solution is 5.0 × 10-5 M in each of these ions: Ag+, SO2, CI, and CO²-. Which precipitate will form? Ag2SO4 (Ksp = 1.12 x 10-5) AgCl (Ksp = 1.77 x 10-1⁰) Ag2CO3 (Ksp = 8.46 x 10-¹2)

Calcium and magnesium ions can occur in our water supplies (e.g. through rocks and geological formations). A sample of tap water was tested and the calcium ion concentration was measured at 2.1E-5M and the magnesium ion concentration was measured at 1.2E-3M. If carbonate ion is added into the tap water, which ion will precipitate out of solution first? Explain your reasoning. The Ksp values of CaCo3 and MgCO3 are 5.0E-9 and 6.8E-6, respectively.

Calculate the amount of precipitate when excess CO2 is bbbled through a solution containing 0.205 mol of Ba(OH)2 according to the equation:  Ba(OH)2 + CO2 --> BaCO3 (MM=197.4g) +H2O (MM=18.02)

A solution is 5.0 x 10-5 M in each of these ions: Ag+, SO;-, CF, and CO?-. Which precipitate will form? Ag,CO3 (Kp = 8.46 × 10-12) Ag,SO4 (Kp = 1.12 × 10-5) AgCI (Kp = 1.77 × 10-19)

A chemistry graduate student is given 100. mL of a 1.30M dimethylamine ((CH3), NH) solution. Dimethylamine is a weak base with K,=5.4 x 10 ". What 2 mass of (CH,) NH,Br should the student dissolve in the (CH,), NH solution to turn it into a buffer with pH = 10.46? You may assume that the volume of the solution doesn't change when the (CH,) NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it 2 to 2 significant digits. x10 ?

a solution contains 0.0036 M Zn^+2 and 0.044 M Fe^+2. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. at what concentration of sulfide ion will a precipitate begin to form? what is the identity of the precipitate? Ksp(Zns)=2.0x10^-25, Ksp(FeS)=6.3x10^-18. a)1.4x10^-16 M, FeS b)1.4x10^-16 M, ZnS c)5.6x10^-24 M, ZnS d)5.6x10^-24 M, FeS e) No precipitate will form at any concentration of sulfide ion.

What is the molar solubility of Ca(OH)2 in the presense of dissolved Cacl2 if the volume of the sample analyzed is 25.00 mL and the initial buret reading is 0.75 mL and the final is 25.80?