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11. Calculate the volume in mL of a 1.420 M NaOH solution required to titrate the following solutions: a. 25.00 mL of a 2.430 M HCl solutionb. 25.00 mL of a 4.500 M H2SO4 solutionc. 25.00 mL of a 1.500 M H3PO4 solution

Question

11. Calculate the volume in mL of a 1.420 M NaOH solution required to titrate the following solutions: 

a. 25.00 mL of a 2.430 M HCl solution
b. 25.00 mL of a 4.500 M H2SO4 solution
c. 25.00 mL of a 1.500 M H3PO4 solution 

 

check_circleAnswer
Step 1

(a)

Volume of NaCl needed to titrate 25.00 mL of 2.430 M HCl solution is determined as follows,

M,V M,V
Molarity of HClxVolume of HCl
Molarity of NaOH
Volume of NaOH
(2.430 M) (25.00 mL) = 42.78 mL
(1.420M)
Volume of NaOH needed = 42.78 mL
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M,V M,V Molarity of HClxVolume of HCl Molarity of NaOH Volume of NaOH (2.430 M) (25.00 mL) = 42.78 mL (1.420M) Volume of NaOH needed = 42.78 mL

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Step 2

(b)

H2SO4 is a diprotic acid. Volume of NaCl needed to titrate 25.00 mL of 4.500 M H...

Balanced equation: H2SO,(aq)
Na,SO, (aq)H0(1)
2NaOH (aq)
IL 10 mL
No. of moles of H2SO, = Molarityx Volume (in L)
-(4.5 M)(0.025 L)= 0.1125 mol H2SO
4
From the equation, 1 mol H,SO4 reacts with 2 mol NaOH
Therefore, in the titration
No. of moles of N2OH reacted = (2x0.1125 mol) = 0.2250 mol N2OH
(0.2250 mol)
No.of mol
0.1584 L= 158.4 mL
Volume of NaOH
Molarity
1.42 M
Volume of NaOH required is 158.4 mL
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Balanced equation: H2SO,(aq) Na,SO, (aq)H0(1) 2NaOH (aq) IL 10 mL No. of moles of H2SO, = Molarityx Volume (in L) -(4.5 M)(0.025 L)= 0.1125 mol H2SO 4 From the equation, 1 mol H,SO4 reacts with 2 mol NaOH Therefore, in the titration No. of moles of N2OH reacted = (2x0.1125 mol) = 0.2250 mol N2OH (0.2250 mol) No.of mol 0.1584 L= 158.4 mL Volume of NaOH Molarity 1.42 M Volume of NaOH required is 158.4 mL

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