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slavikrds [6]
3 years ago
14

You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1

105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point? View Available Hint(s) You are given a solution of (formic acid) with an approximate concentration of 0.20 and you will titrate this with a 0.1105 . If you add 20.00 of to the beaker before titrating, approximately what volume of will be required to reach the end point? 11.1 mL 20.0 mL 72.4 mL 36.2 mL
Chemistry
1 answer:
jeka57 [31]3 years ago
3 0

Answer:

\boxed{\text{36 mL}}

Explanation:

1. Write the balanced chemical equation.

\rm HCOOH + NaOH $ \longrightarrow$ HCOONa + H$_{2}$O

2. Calculate the moles of HCOOH

\text{Moles of HCOOH} =\text{20.00 mL HCOOH } \times \dfrac{\text{0.20 mmol HCOOHl}}{\text{1 mL HCOOH}} = \text{4.00 mmol HCOOH}

3. Calculate the moles of NaOH.

\text{Moles of NaOH = 4.00 mmol HCOOH } \times \dfrac{\text{1 mmol NaOH} }{\text{1 mmol HCOOH}} = \text{4.00 mmol NaOH}

4. Calculate the volume of NaOH

c = \text{4.00 mmol NaOH } \times \dfrac{\text{1 mL NaOH }}{\text{0.1105 mmol NaOH }} = \textbf{36 mL NaOH }\\\\\text{The titration will require }\boxed{\textbf{36 mL of NaOH}}

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