If Ksp of AgCl(s) is 1.77 x 10-10, will a precipitate form when a sample of AgNO3 (aq) ismixed with a sample of NaCl (aq) to make a solution where the concentration of AgNO3(aq) is 0.10 M and NaCl (aq) is 0.090 M? All I know is that if the Q value is higher than the Ksp Value it results in a precipitate.

Suppose 100 mL of 2.0 × 10–4 M Fe(NO3)3is added to 100 mL of 2.0 ×10–5 M KIO3. What is Qsp value? Will it precipitate?

What you expect to observe on mixing 0.1M AgNO3 with 3M H2SO4. 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?

4. Tap water contains the sulfate ion 50 at about 0.00400 mol/L. If 15 mL of 0.00100 mol/L BaCl, is added to 85 mL of tap water, will a precipitate form? Kup of barium sulfate is 1.1 x 10-¹0 (T/1:6)

At what pH will Fe(OH)₃(s) begin to precipitate from 4.45 × 10⁻³ M FeCl₃? Ksp for Fe(OH)₃ is 2.79 × 10⁻³⁹.

(vi) Determine whether a precipitate of AgCI(s) will form on mixing 50.0 mL of 1.0 x 10-4 mol L-1 NaCl with 50.0 mL of 1.0 x 10-6 mol L-1 AGNO3. The Ksp for AgCI(s) is 1.8 x 10-10.

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10M in AgNO3 and 0.075M in NaCl. What will happen once these solutions are mixed? Ksp(AgCl)=1.77•10-10.  A) nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. B) silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl. C) silver chloride will precipitate out of solution, leaving a saturated AgCl solution. D) nothing will happen since NaCl and AgNO3 are both soluble compounds. E) there's not enough information to say anything.

Can you please answer question 15.90 and all of the sub problems and show all of the steps to the solution

What you expect to observe on mixing 0.1M Na2CO3 with 6M NaOH. 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?

The Ksp of PbBr, is 6.60 × 10-6. What is the molar solubility of PbBr, in pure water? molar solubility: 1.181 x10-2 M What is the molar solubility of PbBr, in 0.500 M KBr solution? molar solubility: 2.64 x10¬ M What is the molar solubility of PbBr, in a 0.500 M Pb(NO,), solution? 3.63 x10¬3 molar solubility: M Incorrect