Use the solubility rules listed in Section 8.3B to predict whether each of the following ionic compounds is soluble in water. a. Al(NO 3) 3 e. CuCO 3 b. NaHCO 3 f. (NH 4) 2SO 4 c. Cr(OH) 2 g. Fe(OH) 3 d. LiOHh. (NH 4) 3PO 4

A solution contains 1.45x10-2 M sodium carbonate and 9.94x10-3 M ammonium sulfide. Solid copper(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu²+] = M

Determine the mass, in grams, of precipitate that forms when 608, ml. of 0.499 M Na₂CO, reacts with 882. ml. of 0.455 M Ca(OH)₂. Round your answer to 3 significant figures. Ca(OH)₂ (aq) + Na₂CO, (aq) Caco, O.P - 2NaOH(aq) + CaCO, (s)

1a. For each combination of two aqueous solutions, predict whether or not a precipitate (solid product) will form. Put a check mark by those reactions that WILL form a precipitate. options:   Na2CO3 and CaCl2   NH4NO3 and SrCl2   KI and PbNO3   KBr and NH4Cl   1b. Kidney stones generally form from the double displacement reaction of two salts that form an insoluble compound, a precipitate. Which of the following salts will react in a double displacement reaction with Na3PO4 to form an insoluble precipitate(s):   Potassium chloride (KCl)   Potassium carbonate (K2CO3)   Magnesium sulfate (MgSO4)   Oxalic acid (H2C2O4)   Sodium acetate (CH3CO2Na)   1c. Dibasic sodium phosphate dihydrate (Na2HPO4⋅2H2O) is one of the compounds you may consider using. When it is dissolved in water, which ions will be present in significant amounts in solution? Select all that apply. Na2^+   HPO4^-1   HPO4^-2   PO4^-1…

A solution contains 6.69x10-3 M sodium hydroxide and 1.48x10-2 M ammonium phosphate. Solid chromium(III) acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula B. What is the concentration of chromium(III) ion when this precipitation first begins? [Cr³+] = M

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

Consider the following chemical reaction. 3 Zn(C₂H₃O₂)₂(aq) + 2 Na₃PO₄(aq) → 6 NaC₂H₃O₂(aq) + Zn₃(PO₄)₂(s) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C₂H₃O₂)₂ in 105 mL H₂O. What is the concentration of this zinc acetate solution?

A technician would like to standardize an unknown Ca(OH)2 solution. It takes 22.41 mL of a 0.155 M solution of HCl to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution.  Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2.

3+ The solubility-product constant for Ce(IO3)3 is 3.2 × 10−¹⁰. What is the Ce³+ concentration in a solution prepared by mixing 40.00 mL of 0.0440 M 40.00 mL of a. water? b. 0.0440 M IO3¯? c. 0.280 M IO3¯? M M M 3+ Ce ³+ with

A solution contains 1.47×10-2 M sodium carbonate and 7.31×10-3 M potassium hydroxide. Solid copper(II) nitrate is added slowly to this mixture.A. What is the formula of the substance that precipitates first? formula =    B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu2+] =         M