# If you could help me it would be greatly appreciated, Thanx

Question 1
In a titration, a 20mL sampl of NaOh(aq) was neutralized by 14.9 mL of 0.13 mol/L H2SO4(aq). The concentration of the base is

A. 8.7 mol/L
B. 0.35 mol/L
C. 0.19 mol/L
D. 0.048 mol/L

Question 2

A lab technician diluted a 25.0 mL sample of ethanoic acid, with an initial concentration of 18.0 mol/L, to obtain a molar concentration of 0.500 mol/L. To what volume of water did the technician add the 25 mL of acid? Show complete calculations.

If you could help me it would be greatly appreciated, Thanx

Question 1
In a titration, a 20mL sampl of NaOh(aq) was neutralized by 14.9 mL of 0.13 mol/L H2SO4(aq). The concentration of the base is
H2SO4 + 2NaOH ==> 2H2O+ Na2SO4
mols H2SO4 = L x M = ??

Use the coefficients in the equation to convert mols H2SO4 to mols NaOH.
mols NaOH = ??mol H2SO4 x (2 mol NaOH/1 mol H2SO4 = xx mol NaOH.

Then use the definition of M = mols/L to convert xx mol NaOH to M (the volume is 0.020 L)

A. 8.7 mol/L
B. 0.35 mol/L
C. 0.19 mol/L
D. 0.048 mol/L

Question 2

A lab technician diluted a 25.0 mL sample of ethanoic acid, with an initial concentration of 18.0 mol/L, to obtain a molar concentration of 0.500 mol/L. To what volume of water did the technician add the 25 mL of acid? Show complete calculations

mL x M = mL x M
Show your work if you get stuck and need further assistance.

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