QUESTION 4 Using the solubility rules from Table 61 of your

QUESTION 4 Using the solubility rules from Table 6-1 of your lab manual, fill out the expected results when the starting materials in the chart below react. Place a \"P\" in the box if you expect a precipitate to form between two starting materials, \"g\" if you expect a gas to form, and \"NR\" if you think no reaction will occur. If the product is slightly soluble put a \"p*\". An example is shown below. Example: A P is in the top left cell where Rb2504 and AgNO3 intersect because when these starting materials react, you get the following equations. Molecular Equation: Rb2SO4(a 2 AgNo3(a)2 RbNO3(a+Ag2504(s) Net lonic Equation: 2 Ag (aq) + S042-(aq)Ag2504(s) Since a solid/precipitate is formed as a product, a P has been written in the appropriate cell these starting materials intersect. Starting Materials Rb2504 Cs3PO4 AgNO3 P NH4CI P SrBr2

Solution

Molecular Equation:

Cs₃PO₄ (aq) + 3 AgNO₃ (aq) -------> Ag₃PO₄ (s) + 3 CsNO₃ (aq)

Net Ionic Equation:

PO₄^3- (aq) + 3 Ag⁺ (aq) --------> Ag₃PO₄ (s)

Molecular Equation:

Rb₂SO₄ (aq) + 2 NH₄Cl (aq) --------> 2 RbCl (aq) + (NH₄)₂SO₄ (aq)

The reactants and the products are all soluble and easily ionize; this is a simple double displacement reaction and hence, apparently no reaction (NR) takes place.

Molecular Equation:

Cs₃PO₄ (aq) + 3 NH₄Cl (aq) -------> (NH₄)₃PO₄ (aq) + 3 CsCl (aq)

The reactants and the products are all soluble and easily ionize; this is a simple double displacement reaction and hence, apparently no reaction (NR) takes place.

Molecular Equation:

Rb₂SO₄ (aq) + SrBr₂ (aq) --------> 2 RbBr (aq) + SrSO₄ (s)

Net Ionic Equation:

SO₄^2- (aq) + Sr²⁺ (aq) -------> SrSO₄ (s)

Molecular Equation:

2 Cs₃PO₄ (aq) + 3 SrBr₂ (aq) -------> Sr₃(PO₄)₂ (s) + 6 CsBr (aq)

Net Ionic Equation:

2 PO₄^3- (aq) + 3 Sr²⁺ (aq) --------> Sr₃(PO₄)₂ (s)

Starting Materials

Rb₂SO₄

Cs₃PO₄

AgNO₃

P

P

NH₄Cl

NR

NR

SrBr₂

P

P

Starting Materials	Rb2SO4	Cs3PO4
AgNO3	P	P
NH4Cl	NR	NR
SrBr2	P	P