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3 years ago

Paul determines that the hydrogen ion concentration of his unknown solution is 3.60×10^-5 M. what is the pH of this solution?

Chemistry

1 answer:

vivado [14]3 years ago

4 0

Answer:

Explanation:

The pH of a substance can be found by using the formula

$p H = - log[ H^{ + } ]$

where [ H+ ] is the hydrogen ion concentration of the solution

From the question

[ H + ] = 3.60 × 10^-5 M

So the pH is

$pH = - log(3.60 \times {10}^{ - 5} ) \\ =4.44369749923$

We have the final answer as

Hope this helps you

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Calculate the density of a sample of 1.00 mole of nh3 at 793mmhg and -9.00 c

xeze [42]

0.164 g/L is the density of a sample of 1.00 mole of $NH_3$ at 793mmhg and -9.00 degrees celcius.

<h3>What is density?</h3>

Density is the mass of a unit volume of a material substance. The formula for density is d = $\frac{M}{V}$ , where d is density, M is mass, and V is volume.

Given data:

n = 1.00 mole

P=793 mm hg =1.04342 atm

T=-9.00 degree celcius = -9.00 + 273= 264 K

V=?

Using Ideal Gas Law equation:

PV = n R T

R = gas constant = 0.082057 L-atm/(mol-K)

(1.04342 atm)(V) = 5 X 0.082057 L-atm/(mol-K) X 264 K

V = 103.67 Liters

Now calculate density:

Mole weight of $NH_3$ = 1.00 mole

So, the mass of $NH_3$ = 17.031 g

Density = $\frac{mass}{volume}$

Density = $\frac{17.031 g}{ 103.67 Liters}$

= 0.164 g/L

Hence, 0.164 g/L is the density of a sample of 1.00 mole of $NH_3$ at 793mmhg and -9.00 degrees celcius.

Learn more about the density here:

brainly.com/question/15164682

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8 0

2 years ago

How many molecules are found in 90 grams of Al(OH)3?

jarptica [38.1K]

Answer:

6.95 x 10²³ molecules/particles

Explanation:

First we need to find the total Empirical Mass. We can find this by adding each element's mass together.

Al = 26.982,

O = 15.999

H = 1.008

26.982 + 3(15.999) + 3(1.008) = 78.003.

Now we divide by the mass given (90 grams).

90/78.003 = 1.153801777.

We then take that number and multiply it by avogadro's number (6.022 x 10²³)

1.153801777 x avogadro's number = 6.95 x 10²³

6 0

3 years ago

What would happen if less calcium chloride reacted and more unknown carbonate reacted?

Anit [1.1K]

A white insoluble solid would appeaer

8 0

3 years ago

Calculate the maximum numbers of moles and grams of H₂S that can form when 158 g of aluminum sulfide reacts with 131 g of water:

Phantasy [73]

What is Chemical Reaction?

A chemical reaction is the chemical transformation of one set of chemical components into another.

Main Content

Mass of aluminium sulfide is 158g

Mass of water is 131g

The chemical reaction: $Al_{2}S_{3} +H_{2}O _\to Al(OH)_{3} + H_{2}S$

First, balance the chemical equation

$Al_{2}S_{3} + 6H_{2}O \to 2Al(OH)_{3} + 3H_{2}S$

Aluminium sulfide has a molar mass of 150.16 g/mol and water has a molar mass of 18.02 g/mol. As a result, the moles of aluminum sulfide are computed as follows:

$n_{Al_{2}S_{3} } = \frac{Mass}{Molar mass}\\n_{Al_{2} S_{3} } = \frac{158g}{150.16g/mol} \\n_{Al_{2}S_{3} }=1.05 mol$

From the chemical reaction , the ratio of molar is 3mol $H_{2}S/1 mol Al_{2}S_{3}.$ So, the moles of hydrogen sulfide are:

$n_{H_{2} O} =\frac{131g}{18.02g/mol}$

= 7.26mol

From the chemical reaction, the molar ratio is 3 mol $H_{2}S/6$ mol $H_{2}O.$ So, the moles of hydrogen sulfide are:

Moles of $H_{2}S$ formed = 7.26 mol $H_{2}O \times \frac{3 mol H_{2}S }{6 mol H_{2} O} }$

Th liming reactant is $Al_{2}S_{3}$ beacuse the mass of $Al_{2}S_{3}$ forms less product than water. Therefore, the maximum number of moles of $H_{2}S$ is 3.15 mol. We know that molar mass of $H_{2}S$ is 34.10g/mol. So, the maximum mass of $H_{2}S$ formed is,

$m_{H_{2}S } = n_{H_{2}S } \times$ Molar mass of $H_{2}S$

= 3.15 mol $\times$ 34.10g/mol

= 107.4g

Now, multiplying the number of moles of $Al_{2}S_{3}$ by the molar ratio between $Al_2S_3$ and $H_2O$ which is 6mol $H_2O/1mol$ $Al_2S_3$ we get the number of moles of $H_2O$ reacted.