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3 years ago

8

If the temperature outside is 75oF and the dew point is 75oF what is the humidity?

1 answer:

Serjik [45]3 years ago

8 0

Answer:

in this file you will find it https://xlbrands.com/wp-content/uploads/2014/06/DEW-POINT-CALCULATION-CHARTenglish.pdf

Explanation:

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Calculate the pH of a buffer that is prepared by mixing 25.0 mL of 0.300 M methylamine (CH3NH2) and 0.405 g of methylammonium ch

SVETLANKA909090 [29]

<u>Answer:</u> The pH of the solution is 10.74

<u>Explanation:</u>

<u>For methylammonium chloride:</u>

To calculate the number of moles, we use the equation:

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

Given mass of methylammonium chloride = 0.405 g

Molar mass of methylammonium chloride = 67.52 g/mol

Putting values in above equation, we get:

$\text{Moles of methylammonium chloride}=\frac{0.405g}{67.52g/mol}=0.00599mol$

<u>For methylamine:</u>

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Molarity of methylamine solution = 0.300 M

Volume of solution = 25 mL = 0.025 L

Putting values in above equation, we get:

$0.300M=\frac{\text{Moles of methylamine}}{0.025L}\\\\\text{Moles of methylamine}=(0.300mol/L\times 0.025L)=0.0075mol$

Total volume of the solution = [25 + 500] = 525 mL = 0.525 L (Conversion factor: 1 L = 1000 mL)

To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:

$pOH=pK_b+\log(\frac{[salt]}{[base]})$

$pOH=pK_b+\log(\frac{[CH_3NH_3^+Cl^-]}{[CH_3NH_2]})$

We are given:

$pK_b$ = negative logarithm of base dissociation constant of methylamine = 3.36

$[CH_3NH_2]=\frac{0.0075}{0.525}$

$[CH_3NH_3^+Cl^-]=\frac{0.00599}{0.525}$

pOH = ?

Putting values in above equation, we get:

$pOH=3.36+\log (\frac{(0.00599/0.525)}{(0.0075/0.525)}\\\\pOH=3.26$

To calculate the pH of the solution, we use the equation:

$pH+pOH=14\\\\pH=14-3.26=10.74$

Hence, the pH of the solution is 10.74

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