1-A HCl solution is titrated with a NaOH solution of known concentration. How mu

Question

1-A HCl solution is titrated with a NaOH solution of known concentration. How much volume of NaOH 0.132 M is necessary to neutralize 10.00 mL of HCl 0.200 M?

2-A 5.00 mL sample of toilet cleaner weighs 4.902 g. When titrated, those 5.00 mL of the household product need 25.50 mL of NaOH 0.506 M for the end point to be reached.

What is the density of the toilet cleaner?

How many moles of HCl are contained in those 5.00 mL of household product?

What mass of HCl is contained in those 5.00 mL of household product?

What is the molarity of the toilet cleaner?

What is the mass percentage of HCl in the toilet cleaner?

Explanation / Answer

1)

Balanced chemical equation is:

HCl + NaOH ---> NaCl + H2O

Here:

M(HCl)=0.2 M

M(NaOH)=0.132 M

V(HCl)=10.0 mL

According to balanced reaction:

1*number of mol of HCl =1*number of mol of NaOH

1*M(HCl)*V(HCl) =1*M(NaOH)*V(NaOH)

1*0.2 M *10.0 mL = 1*0.132M *V(NaOH)

V(NaOH) = 15.2 mL

Answer: 15.2 mL

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