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PbSO4 O Pb(NO3)2 (ag)+ Na2SO4 (ag)→PBSO4(s) + 2NaNO3(ag) O Pb(NO3)2(aq) + BaSO4 (s)→PBSO(s) + Ba(NO3)2 (aq) O PbS(s) + H2SO4(ag)→PbSO4(s)+ H2S(ag) O PbO(s) + H2SO4(ag)→PbSO4 (s)+ H2O(1)

PbSO4 O Pb(NO3)2 (ag)+ Na2SO4 (ag)→PBSO4(s) + 2NaNO3(ag) O Pb(NO3)2(aq) + BaSO4 (s)→PBSO(s) + Ba(NO3)2 (aq) O PbS(s) + H2SO4(ag)→PbSO4(s)+ H2S(ag) O PbO(s) + H2SO4(ag)→PbSO4 (s)+ H2O(1)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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How would you prepare the following substances by a precipitation reaction?

a) PbSO4

image attached

b)Mg3(PO4)2
 image attached 

c) ZnCrO4

**Lead(II) Sulfate (PbSO₄) Reactions** Choose the correct chemical reaction that results in the formation of lead(II) sulfate (PbSO₄): 1. \( \text{Pb(NO}_3\text{)}_2(aq) + \text{Na}_2\text{SO}_4(aq) \rightarrow \text{PbSO}_4(s) + 2\text{NaNO}_3(aq) \) 2. \( \text{Pb(NO}_3\text{)}_2(aq) + \text{BaSO}_4(s) \rightarrow \text{PbSO}_4(s) + \text{Ba(NO}_3\text{)}_2(aq) \) 3. \( \text{PbS}(s) + \text{H}_2\text{SO}_4(aq) \rightarrow \text{PbSO}_4(s) + \text{H}_2\text{S}(aq) \) 4. \( \text{PbO}(s) + \text{H}_2\text{SO}_4(aq) \rightarrow \text{PbSO}_4(s) + \text{H}_2\text{O}(l) \) Each reaction represents a different method of synthesizing lead(II) sulfate under varying conditions and from different precursor compounds.
Transcribed Image Text:**Lead(II) Sulfate (PbSO₄) Reactions** Choose the correct chemical reaction that results in the formation of lead(II) sulfate (PbSO₄): 1. \( \text{Pb(NO}_3\text{)}_2(aq) + \text{Na}_2\text{SO}_4(aq) \rightarrow \text{PbSO}_4(s) + 2\text{NaNO}_3(aq) \) 2. \( \text{Pb(NO}_3\text{)}_2(aq) + \text{BaSO}_4(s) \rightarrow \text{PbSO}_4(s) + \text{Ba(NO}_3\text{)}_2(aq) \) 3. \( \text{PbS}(s) + \text{H}_2\text{SO}_4(aq) \rightarrow \text{PbSO}_4(s) + \text{H}_2\text{S}(aq) \) 4. \( \text{PbO}(s) + \text{H}_2\text{SO}_4(aq) \rightarrow \text{PbSO}_4(s) + \text{H}_2\text{O}(l) \) Each reaction represents a different method of synthesizing lead(II) sulfate under varying conditions and from different precursor compounds.
**Chemical Reactions for the Formation of Mg\(_3\)(PO\(_4\))\(_2\):** 1. **Reaction 1:** - Equation: \(3\text{Mg(OH)}_2(s) + 2\text{H}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 6\text{H}_2\text{O}(l)\) 2. **Reaction 2:** - Equation: \(3\text{MgCO}_3(s) + 2\text{H}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 3\text{H}_2\text{O}(l) + 3\text{CO}_2(g)\) 3. **Reaction 3:** - Equation: \(3\text{MgCl}_2(aq) + 2\text{K}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 6\text{KCl}(aq)\) 4. **Reaction 4:** - Equation: \(3\text{MgCO}_3(s) + 2\text{K}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 3\text{K}_2\text{CO}_3(aq)\) Each equation represents a different method of synthesizing magnesium phosphate (\( \text{Mg}_3(\text{PO}_4)_2 \)) through various starting materials and reactions.
Transcribed Image Text:**Chemical Reactions for the Formation of Mg\(_3\)(PO\(_4\))\(_2\):** 1. **Reaction 1:** - Equation: \(3\text{Mg(OH)}_2(s) + 2\text{H}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 6\text{H}_2\text{O}(l)\) 2. **Reaction 2:** - Equation: \(3\text{MgCO}_3(s) + 2\text{H}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 3\text{H}_2\text{O}(l) + 3\text{CO}_2(g)\) 3. **Reaction 3:** - Equation: \(3\text{MgCl}_2(aq) + 2\text{K}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 6\text{KCl}(aq)\) 4. **Reaction 4:** - Equation: \(3\text{MgCO}_3(s) + 2\text{K}_3\text{PO}_4(aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2(s) + 3\text{K}_2\text{CO}_3(aq)\) Each equation represents a different method of synthesizing magnesium phosphate (\( \text{Mg}_3(\text{PO}_4)_2 \)) through various starting materials and reactions.
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