When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which of the following is correct for this titration?

Chemistry

1 answer:

alisha [4.7K]3 years ago

8 0

Answer:

c) B, C

Explanation:

NaOH(aq) + HBr(aq) -----> NaBr(aq) +H2O(l)

1) concentration of acid CA= 0.05 M

Concentration of base CB= 0.1 M

Volume of acid VA= 25.00ml

Volume of base VB= unknown

Number of moles of acid NA= 1

Number of moles of base NB= 1

CAVA/CBVB = NA/NB

CAVANB =CBVBNA

VB= CAVANB/CB NB

VB= 0.05 × 25 × 1/ 0.1 ×1

VB= 12.5 ML

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Serggg [28]

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3 years ago

Which solution is more concentrated?

deff fn [24]

2 moles of NaOH dissolved in 1 litre of solution is the solution with more concentration.

Answer: Option A

<u>Explanation:</u>

Concentration of solution is the measure of the amount of solute dissolved in the solvent of the solution. So this is measured using the molarity of the solution. Molarity is determined as the number of moles of the solute present in the given amount of solvent.

$\text {Molarity}=\frac{\text {Moles of solute}}{\text {Amount of solvent }}$

In this present case, the option A gives the molarity of 2 M as

$\text {Molarity}=\frac{2}{1}=2 M$

But the second option, mass of NaOH is given. So we have to determine the molarity. First we have to find the molar mass of NaOH. We know that 1 mole of NaOH will contain 40 g/mole.

1 g of NaOH = 40 g of NaOH

1 g of NaOH = 1/40 moles

So 2 g of NaOH will contain $\frac{2 g}{40 g/mole}$ which is equal to 0.05 moles of NaOH.