Q. The neutralization of formic acid by NaOH produces.

Q: What are the products when formic acid \mathrm{HCOOH} is neutralized by \mathrm{NaOH} ?

The products are sodium formate \mathrm{HCOONa} and water \mathrm{H_2O} .

Q: What species forms the conjugate base during neutralization?

\mathrm{HCOO^-} is the conjugate base produced after deprotonation by \mathrm{OH^-} , then it pairs with \mathrm{Na^+} .

Q: If you start with excess \mathrm{NaOH} , what ions remain after completion?

You’ll have leftover \mathrm{OH^-} , and most \mathrm{HCOOH} converts to \mathrm{HCOO^-} as \mathrm{HCOONa} .

Q: If you start with excess \mathrm{HCOOH} , what’s left at the end?

Leftover \mathrm{HCOOH} remains, along with some \mathrm{HCOO^-} , giving an acidic solution.

Answer

Formic acid is a weak acid with formula \( \mathrm{HCOOH} \). Neutralizing it with sodium hydroxide gives a salt and water.

Balanced reaction:

\[
\mathrm{HCOOH + NaOH \rightarrow HCOONa + H_2O}
\]

Products formed:

The neutralization produces sodium formate \(\mathrm{HCOONa}\) and water \(\mathrm{H_2O}\).

Detailed Explanation

This question is asking for the products of a neutralization reaction between formic acid and sodium hydroxide (NaOH).

Step 1: Write the balanced chemical equation.

Formic acid is the weak acid with formula \( \mathrm{HCOOH} \). Sodium hydroxide is the base with formula \( \mathrm{NaOH} \).

Neutralization of an acid by a base typically produces a salt and \( \mathrm{H_2O} \).

The reaction is:

\[
\mathrm{HCOOH + NaOH \rightarrow HCOONa + H_2O}
\]

Step 2: Identify the products.

From the balanced equation, the products are:

\( \mathrm{HCOONa} \) which is sodium formate, and \( \mathrm{H_2O} \) which is water.

Final Answer (products): sodium formate and water, i.e.,

\[
\mathrm{HCOOH + NaOH \rightarrow HCOONa + H_2O}
\]

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General Chemistry FAQs

What are the products when formic acid \( \mathrm{HCOOH} \) is neutralized by \( \mathrm{NaOH} \)?

The products are sodium formate \( \mathrm{HCOONa} \) and water \( \mathrm{H_2O} \).

Write the balanced neutralization equation for \( \mathrm{HCOOH} \) with \( \mathrm{NaOH} \).

\[ \mathrm{HCOOH + NaOH \rightarrow HCOONa + H_2O} \]

Is the neutralization reaction exothermic or endothermic?

It is typically exothermic for strong base plus weak acid neutralization. Heat is released as ions form in water.

What species forms the conjugate base during neutralization?

\( \mathrm{HCOO^-} \) is the conjugate base produced after deprotonation by \( \mathrm{OH^-} \), then it pairs with \( \mathrm{Na^+} \).

If you start with excess \( \mathrm{NaOH} \), what ions remain after completion?

You’ll have leftover \( \mathrm{OH^-} \), and most \( \mathrm{HCOOH} \) converts to \( \mathrm{HCOO^-} \) as \( \mathrm{HCOONa} \).

If you start with excess \( \mathrm{HCOOH} \), what’s left at the end?

Leftover \( \mathrm{HCOOH} \) remains, along with some \( \mathrm{HCOO^-} \), giving an acidic solution.

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Q. The neutralization of formic acid by NaOH produces.

Answer

Detailed Explanation

General Chemistry FAQs

What are the products when formic acid \( \mathrm{HCOOH} \) is neutralized by \( \mathrm{NaOH} \)?

Write the balanced neutralization equation for \( \mathrm{HCOOH} \) with \( \mathrm{NaOH} \).

Is the neutralization reaction exothermic or endothermic?

What species forms the conjugate base during neutralization?

If you start with excess \( \mathrm{NaOH} \), what ions remain after completion?

If you start with excess \( \mathrm{HCOOH} \), what’s left at the end?

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