Question

What volume of acetic acid of density 1.10g/cm3 is needed to react with 250 mL of 0.50M Stronuim hydroxide?

Answer 1

`V=13.6cm^3`

Step-by-step explanation:

Hello,

In this case, given the reaction in which the acetic acid reacts with strontium hydroxide to yield water and strontium acetate:

`2CH_3COOH+Sr(OH)_2\rightarrow Sr(CH_3COO)_2+2H_2O`

The first step here is to compute the moles of strontium hydroxide that are reacting given its volume in liters (0.250 L) and concentration:

`n_(Sr(OH)_2)=0.50mol/L*0.250L=0.125molSr(OH)_2`

Next, considering the 1:2 mole ratio between the strontium hydroxide and the acetic acid (molar mass = 60 g/mol) we compute the grams of acid that are consumed:

`m_(CH_3COOH)=0.125molSr(OH)_2*(2molCH_3COOH)/(1molSr(OH)_2) *(60gCH_3COOH)/(1molCH_3COOH)\\ \\m_(CH_3COOH)=15gCH_3COOH`

Then, by using the density of the acetic acid, we compute the volume:

`V=(m)/(\rho)=(15g)/(1.10g/cm^3) \\ \\V=13.6cm^3`

Best regards.