Answer:
The molarity of the strong base is 0.625 M
Which procedural error will result in a strong base molarity that is too high?
⇒ Using a buret with a tip filled with air rather than the H2SO4 solution
Explanation:
<u>Step 1:</u> Data given
Molarity of H2SO4 = 0.250 M
The initial buret reading is 5.00 mL
The final reading is 30.00 mL
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<u>Step 2:</u> Calculate volume of H2SO4 used
30.00 mL - 5.00 mL = 25.00 mL
<u>Step 3:</u> Calculate moles of H2SO4
0.250 M = 0.250 mol/L
Since there are 2 H+ ions per H2SO4
0.250 mol/L * 2 = 0.500 mol/L
The number of moles H2SO4 = 0.500 mol/L * 0.025 L
Number of moles H2SO4 = 0.0125 mol
<u>Step 4</u>: Calculate moles of OH-
For 1 mol H2SO4, we need 1 mol of OH-
For 0.0125 mol of H2SO4, we have 0.0125 mol of OH-
<u>Step 5</u>: Calculate the molarity of the strong base
Molarity = moles / volume
Molarity OH- = 0.0125 mol / 0.02 L
Molarity OH - = 0.625 M
Which procedural error will result in a strong base molarity that is too high?
⇒ Using a buret with a tip filled with air rather than the H2SO4 solution
