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what is the molarity of H2SO4 (aq) in a rainwater if 22.5 mL of 0.100 M NaOH(aq) are needed to neutralize to sample of 25.0 mL rainwater. The balanced chemical equation of for this acid-base reaction is:                                            H2SO4(aq) + 2NaOH(aq) →  Na2SO4(aq) + H20(l)Step1. Determine the number of moles of the base used to neutralize the acid. n(NaOH)= MxV=Step2. Determine the number of moles of the H2SO4  that reacted by using the balanced chemical equation.H2SO4, mol ll Step3. Determine the molarity of the H2so4 in the rainwater:M(H2SO4)=

what is the molarity of H2SO4 (aq) in a rainwater if 22.5 mL of 0.100 M NaOH(aq) are needed to neutralize to sample of 25.0 mL rainwater. The balanced chemical equation of for this acid-base reaction is:

                                           H2SO4(aq) + 2NaOH(aq) →  Na2SO4(aq) + H20(l)

Step1. Determine the number of moles of the base used to neutralize the acid.

n(NaOH)= MxV=

Step2. Determine the number of moles of the H2SO4  that reacted by using the balanced chemical equation.

H2SO4, mol ll

Step3. Determine the molarity of the H2so4 in the rainwater:

M(H2SO4)=

 
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