Question

8. What is the molarity of a CsOH solution if 30.0 mL of the solution is neutralized by 26.4 mL 0.25 M HBr solution (Hint: Ma x Va = Mb x Vb. Rearrange to solve for Mb)?
Ma = Molarity of Acid (M – mol/L)
Va = Volume of Acid (mL needs to be converted to L)
Mb = Molarity of Base (M – mol/L)
Vb = Volume of Base (mL needs to be converted to L)
CsOH = Base = What’s the molarity of the Base? = Mb
HBr = Acid = What’s the molarity of the acid? = Ma
Does the problem give you a volume for the acid? = Va
Does the problem give you a volume for the base? = Vb

HBr + CsOH = CsBr + H2O 

Answer 1

Answer:

Remember, Molarity is moles of solute divided by Liters of solution. ... Hint: Don't forget to convert mL to L and use the formula Ma x Va = Mb x Vb. You are ... 8 What is the molarity of a CsOH solution if 30.0 mL of the solution is neutralized by 26.4 mL 0.25 M HBr solution ( Hint: Ma x Va = Mb x Vb. Rearrange to solve for Mb )? ..

Explanation:

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Answer 2

Answer:

0.22M

Explanation:

The equation for the reaction is given below:

HBr + CsOH —> CsBr + H2O

From the above, the mole ratio of the acid to base is 1.

Data obtained from the question include:

Ma = 0.25M

Va = 26.4mL

Mb =?

Vb = 30mL

Ma x Va = Mb x Vb

Mb = (Ma x Va) / Vb

Mb = ( 0.25x26.4 ) / 30

Mb = 0.22M

Therefore, the molarity of CsOH is 0.22M