Q4.51P If 25.98 mL of a standard 0.1180... [FREE SOLUTION]

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Chapter 4: Q4.51P (page 180)

If 25.98 mL of a standard 0.1180 M KOH solution reacts with 52.50 mL of solution, what is the molarity of the acid solution?

Short Answer

Expert verified

The molarity of the acid solution is 0.058 M.

Step by step solution

Write the balanced molecular equation

The reaction of potassium hydroxide and acetic acid is shown below.

$K O H (a q) + C H_{3} C O O H (a q) 鈫� C H_{3} C O O K (a q) + H_{2} O (l)$

Calculate the moles of acetic acid

Given values are:

$v o l u m e o f s t a n d a r d 0.1180 M K O H s o l u t i o n = 25.98 m l v o l u m e o f a c e t i c a c i d s o l u t i o n = 52.50 m l$

Moles of acetic acid is:

$\begin{array}{rcl} m o l e s o f a c e t i c a c i d & = & 25.98 m l K O H 脳 \frac{1 l i t}{1000 m l} 脳 \frac{0.1180 m o l K O H}{1 l i t K O H s o l u t i o n} 脳 \frac{1 m o l C H_{3} C O O H}{1 m o l K O H} \\ = & 3.07 x 10^{- 3} m o l 鈥� C H_{3} C O O H \end{array}$

Calculate the molarity of acetic acid

The molarity of the acid solution is:

$m o l a r i t y o f a c i d s o l u t i o n = \frac{m o l e s o f a c e t i c a c i d}{v o l u m e o f a c e t i c a c i d}$

The molarity of acetic acid is calculated as:

$= \frac{3.07 x 10^{- 3} m o l C H_{3} C O O H}{(52.50 m l) (\frac{1 l i t}{1000 m l})} = 0.058 M C H_{3} C O O H s o l u t i o n$

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91影视

If 25.98 mL of a standard 0.1180 M KOH solution reacts with 52.50 mL of solution, what is the molarity of the acid solution?

Short Answer

Step by step solution

Write the balanced molecular equation

Calculate the moles of acetic acid

Calculate the molarity of acetic acid

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