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(B) The reaction involves the consumption of $OH^-$ ions in the first step.Adding $HCl$ introduces $H^+$ ions into the solution.The $H^+$ ions react w

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Decreases

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(B) The reaction involves the consumption of $OH^-$ ions in the first step.Adding $HCl$ introduces $H^+$ ions into the solution.The $H^+$ ions react with $OH^-$ ions according to the neutralization reaction: $H^+_{(aq)} + OH^-_{(aq)} 	o H_2O_{(l)}$.This decreases the concentration of $OH^-$ ions in the reaction mixture.Since $OH^-$ is a reactant in the first step,the rate of the reaction,which depends on the concentration of $OH^-$,will decrease.

For the following reaction in aqueous solution,what happens to the rate of reaction if $HCl$ is added?
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$

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For the following reaction in aqueous solution,what happens to the rate of reaction if $HCl$ is added?$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$