chemistry question, titrations

Chemistry
Tutor: None Selected Time limit: 1 Day

a 30.0mL sample of .220M sulfuric acid is titrated with potassium hydroxide. if it takes 26.4mL of base solution to reach the endpoint, what is the molarity of the base solution?

Apr 21st, 2015

Firstly, we can write down the chemical balanced equation as follow:

H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)

Conversion of units:
30.0 mL = 0.03 L
26.4 mL = 0.0264 L

The moles of sulfuric acid used can be calculated by:

nacid = Macid x Vacid = (0.220 M) x (0.03 L) = 6.6 x 10-3 mol

According to the balanced equation, since 1 mol of H2SO4 is reacted with 2 mol of KOH, we have that the moles of potassium hydroxide is equal to

nbase = 2 x 6.6 x 10-3 mol = 1.32 x 10-2 mol

Finally, the molarity of the 26.4mL base solution is determined by:

Mbase = nbase/ Vbase = ( 1.32 x 10-2 mol) / (0.0264 L) = 0.500 M

Answer: 0.500 M



Apr 21st, 2015

Studypool's Notebank makes it easy to buy and sell old notes, study guides, reviews, etc.
Click to visit
The Notebank
...
Apr 21st, 2015
...
Apr 21st, 2015
Dec 4th, 2016
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle
Final Answer

Secure Information

Content will be erased after question is completed.

check_circle
Final Answer