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Chapter 16: Problem 9

Fill in the blanks in the following table. (a) \(\mathrm{CoCO}_{3}\) (b) \(\mathrm{LaF}_{3}\) (c) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Short Answer

Expert verified
Question: Identify the name, type, charges, and formula units for the following compounds: (a) CoCO3 (b) LaF3 (c) Ba3(PO4)2 Answer: (a) Cobalt(II) Carbonate, Ionic Compound, Co^2+ and CO3^2-, CoCO3 (b) Lanthanum(III) Fluoride, Ionic Compound, La^3+ and F^-, LaF3 (c) Barium Phosphate, Ionic Compound, Ba^2+ and PO4^3-, Ba3(PO4)2

Step by step solution

01

(a) CoCO3: Name of Compound

Cobalt(II) Carbonate
02

(a) CoCO3: Type of Compound

Ionic Compound
03

(a) CoCO3: Charges

Cobalt(II) has a charge of +2 (Co^2+), while carbonate (CO3) has a charge of -2 (CO3^2-).
04

(a) CoCO3: Formula Unit

As the charges balance each other out, the formula unit is CoCO3.
05

(b) LaF3: Name of Compound

Lanthanum(III) Fluoride
06

(b) LaF3: Type of Compound

Ionic Compound
07

(b) LaF3: Charges

Lanthanum(III) has a charge of +3 (La^3+), while fluoride (F) has a charge of -1 (F^-).
08

(b) LaF3: Formula Unit

To balance the charges, we need three fluoride ions for each lanthanum ion; the formula unit is LaF3.
09

(c) Ba3(PO4)2: Name of Compound

Barium Phosphate
10

(c) Ba3(PO4)2: Type of Compound

Ionic Compound
11

(c) Ba3(PO4)2: Charges

Barium (Ba) has a charge of +2 (Ba^2+), while phosphate (PO4) has a charge of -3 (PO4^3-).
12

(c) Ba3(PO4)2: Formula Unit

To balance the charges, we need three barium ions and two phosphate ions; the formula unit is Ba3(PO4)2.

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Most popular questions from this chapter

A solution is made up by adding \(0.925 \mathrm{~g}\) of silver(I) nitrate and \(6.25 \mathrm{~g}\) of magnesium nitrate to enough water to make \(375 \mathrm{~mL}\) of solution. Solid sodium carbonate is added without changing the volume of the solution. (a) Which salt, \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) or \(\mathrm{MgCO}_{3}\), will precipitate first? (b) What is the concentration of the carbonate ion when the first salt starts to precipitate?

Consider the following solubility data for calcium oxalate \(\left(\mathrm{Ca} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) : $$ \begin{aligned} &K_{s p} \text { at } 25^{\circ} \mathrm{C}=4 \times 10^{-9} \\ &K_{s p} \text { at } 95^{\circ} \mathrm{C}=1 \times 10^{-8} \end{aligned} $$ Five hundred mL of a saturated solution is prepared at \(95^{\circ} \mathrm{C}\). How many milligrams of \(\mathrm{CaC}_{2} \mathrm{O}_{4}\) will precipitate when the solution is cooled to \(25^{\circ} \mathrm{C}\) ? (Assume that supersaturation does not take place.)

Write an overall net ionic equation and calculate \(K\) for the reaction where \(\mathrm{CuCl}\left(K_{s p}=1.9 \times 10^{-7}\right)\) is dissolved by \(\mathrm{NaCN}\) to form \(\left[\mathrm{Cu}(\mathrm{CN})_{2}\right]^{-}\) \(\left(K_{f}=1.0 \times 10^{16}\right)\).

Cadmium(II) chloride is added to a solution of potassium hydroxide with a \(\mathrm{pH}\) of \(9.62 .\left(K_{\mathrm{sp}} \mathrm{Cd}(\mathrm{OH})_{2}=2.5 \times 10^{-14}\right)\) (a) At what concentration of \(\mathrm{Cd}^{2+}\) does a precipitate first start to form? (b) Enough cadmium(II) chloride is added to make [Cd \(\left.^{2+}\right]=\) \(0.0013 M\). What is the \(\mathrm{pH}\) of the resulting solution? (c) What percentage of the original hydroxide ion is left in solution?

Predict what effect each of the following has on the position of the equilibrium $$ \mathrm{PbCl}_{2}(s) \rightleftharpoons \mathrm{Pb}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \quad \Delta H=23.4 \mathrm{~kJ} $$ (a) addition of \(1 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution (b) increase in temperature (c) addition of \(\mathrm{Ag}^{+}\), forming \(\mathrm{AgCl}\) (d) addition of \(1 M\) hydrochloric acid
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