How many milliliters of 0.139 M HCl would be required to titrate 6.33 g KOH?

Question

anonymous · Answer

@aaronq

aaronq · Answer

There are two ways of doin this question, the first is the formal way using stoichiometry. You write an equation, balance it, convert the reactant(s) to moles and solve.

The second is sort of a shortcut, knowing that they both produce 1 mole of acid or base, respectively, you can use:

$\sf\huge  M_{acid}V_{acid}=M_{base}V_{base}$ 

it works out to the same thing

aaronq · Answer

M is molarity and V is volume

anonymous · Answer

When i tried that, it didn't work. It is in grams @aaronq

aaronq · Answer

oh crap i didn't read the question right lol

so the formula would be 

$\sf M_{acid}V_{acid}=n_{base}$

where n is moles

anonymous · Answer

oh lol ty

anonymous · Answer

We dont know the volume of the acid lol but i solved it using stoich.

aaronq · Answer

well that's what you're solving for

convert the mass of KOH to moles, use the molarity of acid, then you only have 1 variable, the volume of acid