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trapecia [35]
3 years ago
11

Given the following equation, how many grams of PbCO3 will dissolve when exactly 1.0 L of 1.00 M H+ is added to 6.00 g of PbCO3?

Chemistry
2 answers:
9966 [12]3 years ago
4 0
Calculating for the moles of H+
1.0 L x (1.00 mole / 1 L ) = 1 mole H+

From the given balanced equation, we can use the stoichiometric ratio to solve for the moles of PbCO3:
1 mole H+ x (1 mole PbCO3 / 2 moles H+) = 0.5 moles PbCO3

Converting the moles of PbCO3 to grams using the molecular weight of PbCO3
0.5 moles PbCO3 x (267 g PbCO3 / 1 mole PbCO3) = 84.5 g PbCO3
BARSIC [14]3 years ago
3 0

Answer: 6 grams of lead carbonate wlll get easily dissolve in 1 L of 1.0 M H^+ solution.

Explanation:

PbCO_3(s)+2H^+(aq)\rightarrow Pb^2+(aq)+H_2O(l)+CO_2(g)

Moles of H^+ (n):

1.0 M=\frac{\text{mole of }H^+}{\text{Volume of the solution is L}}=\frac{n}{1 L}

n = 1 mole

According to reaction 2 moles of H^+ dissolves 1 mole of PbCO_3 then , 1 mole will dissolve ;\frac{1}{2}\times 1 moles of PbCO_3 that is 0.5 moles

Mass of the compund:

=Number of moles of compound × Molar mass of compound

Mass of dissolved PbCO_3:

=0.5 mole\times 267.21 g/mol=133.605 g

1 L of 1.0 M H^+ solution can dissolve 133.605 grams of lead carbonate. So, 6 grams of lead carbonate wlll get easily dissolve in 1 L of 1.0 M H^+ solution.

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<em></em>

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