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Alisiya [41]
3 years ago
12

If I have 15.40mL of 1.4M HBr(aq) and add 22.10mL KOH what is the molarity ofKOH being used?​

Chemistry
1 answer:
postnew [5]3 years ago
8 0

The molarity of KOH is 0.98 M.

<u>Explanation:</u>

KOH + HBr →KBr + H₂O

As per the above reaction, equal moles of KBr and HBr reacts to form 1 mole of KBr and 1 mole of water. We have to find the molarity of KOH by using the law of Volumetric analysis using the equation as,

V1M1 = V2M2

Here V1 and M1 are the volume and molarity of HBr.

V2 and M2 are the volume and molarity of KOH .

We can find the molarity of KOH as,

$ M2= \frac{V1\times M1}{V2}

Plugin the values as,

$ M2 = \frac{15.40 ml \times 1.4 M}{22.10 ml}

    =  0.98 M

So the molarity of KOH is 0.98 M.

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Mixing of salt is physical change.

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Chemical change:

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7 0
2 years ago
10. Write the word equation of the following skeleton equation.
Aloiza [94]

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4 0
3 years ago
9) After lab, all of Darrel’s friends looked at his data and laughed and laughed. They told him that he was 30.8% too low in the
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3 0
3 years ago
Read 2 more answers
Cho m gam FeO tác dụng hết với dung dịch H2SO4, thu được 200 ml dung dịch FeSO4 1M. Giá trị của m là
BaLLatris [955]

<u>Answer:</u> The mass of FeO required is 14.37 g

<u>Explanation:</u>

Molarity is calculated by using the equation:

\text{Molarity}=\frac{\text{Moles}}{\text{Volume}} ......(1)

We are given:  

Molarity of iron (II) sulfate = 1 M

Volume of solution = 200 mL = 0.200 L (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:

\text{Moles of }FeSO_4=(1mol/L\times 0.200L)=0.200mol

The chemical equation for the reaction of FeO with sulfuric acid follows:

FeO+H_2SO_4\rightarrow FeSO_4+H_2O

By stoichiometry of the reaction:

If 1 mole of iron (II) sulfate is produced by 1 mole of FeO

So, 0.200 moles of iron (II) sulfate will produce = \frac{1}{1}\times 0.200=0.200mol of FeO

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

We know, molar mass of FeO = 71.84 g/mol

Putting values in above equation, we get:

\text{Mass of }FeO=(0.200mol\times 71.84g/mol)=14.37g

Hence, the mass of FeO required is 14.37 g

4 0
3 years ago
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