Chemistry, 02.09.2019 18:20 aubreyfoster

Determine the molarity for each of the following solution solutions:
(a)1.457 mol of kcl in 1.500 l of solution
(b) 0.515 gram ofh2so4, in 1.00 l of solution
(c) 20.54 g of al(no3)3 in 1575 ml of solution
(d)2.76 kg ofcuso4.5h2o in 1.45 l of solution
(e)0.005653 mol ofbr2 in 10.00 ml of solution
(f) 0.000889 g of glycine, c2h5no2, in 1.05 ml of solution

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Answer from: jadenweisman1

Answer :

(a)The molarity of KCl solution is, 0.9713 mole/L

(b)The molarity of H_2SO_4 solution is, 0.00525 mole/L

(c)The molarity of Al(NO_3)_3 solution is, 0.0612 mole/L

(d)The molarity of CuSO_4.5H_2O solution is, 7.61 mole/L

(e)The molarity of Br_2 solution is, 0.0565 mole/L

(f)The molarity of C_2H_5NO_2 solution is, 0.0113 mole/L

Explanation :

(a) 1.457 mol of KCl in 1.500 L of solution

Formula used :

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Solute is KCl.

$\text{Molarity of the solution}=\frac{1.457mole}{1.500L}=0.9713mole/L$

The molarity of KCl solution is, 0.9713 mole/L

(b) 0.515 gram of H_2SO_4 , in 1.00 L of solution

Formula used :

$\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$

Solute is H_2SO_4

Molar mass of H_2SO_4 = 98 g/mole

$\text{Molarity of the solution}=\frac{0.515g}{98g/mole\times 1.00L}=0.00525mole/L$

The molarity of H_2SO_4 solution is, 0.00525 mole/L

Formula used :

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

Solute is Al(NO_3)_3

Molar mass of Al(NO_3)_3 = 213 g/mole

$\text{Molarity of the solution}=\frac{20.54g\times 1000}{213g/mole\times 1575L}=0.0612mole/L$

The molarity of Al(NO_3)_3 solution is, 0.0612 mole/L

(d) 2.76 kg of CuSO_4.5H_2O in 1.45 L of solution

Formula used :

$\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$

Solute is CuSO_4.5H_2O

Molar mass of CuSO_4.5H_2O = 250 g/mole

$\text{Molarity of the solution}=\frac{2760g}{250g/mole\times 1.45L}=7.61mole/L$

The molarity of CuSO_4.5H_2O solution is, 7.61 mole/L

(e) 0.005653 mol of Br_2 in 10.00 ml of solution

Formula used :

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$

Solute is Br_2 .

$\text{Molarity of the solution}=\frac{0.005653mole\times 1000}{10.00L}=0.0565mole/L$

The molarity of Br_2 solution is, 0.0565 mole/L

(f) 0.000889 g of glycine, C_2H_5NO_2 , in 1.05 mL of solution

Formula used :

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

Solute is C_2H_5NO_2

Molar mass of C_2H_5NO_2 = 75 g/mole

$\text{Molarity of the solution}=\frac{0.000889g\times 1000}{75g/mole\times 1.05L}=0.0113mole/L$

The molarity of C_2H_5NO_2 solution is, 0.0113 mole/L

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Determine the molarity for each of the following solution solutions:
(a)1.457 mol of kcl in...

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