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2 years ago

Calculate the pH of a solution whose H3O+ concentration is 2.1 x 10-3 M. Is the solution acidc, basic, or neutral?

Chemistry

1 answer:

Leona [35]2 years ago

5 0

Answer:

Option A, The pH of the solution is 2.7 and the solution is acidic

Explanation:

As we know,

pH = - log [H3O+]

Substituting the given values, we get

pH = - log [2.1 x 10-3 M]

pH = - (-2.678)

pH = 2.678 or 2.7

The solution is acidic as pH value is less than 7

Hence, option A is correct

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Nesterboy [21]

Answer:

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Explanation:

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3 years ago

In atomic science, the z number refers to the number of __________ in the nucleus of an atom.

Sliva [168]

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3 years ago

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kiruha [24]

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2 years ago

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goblinko [34]

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3 years ago

Read 2 more answers

What is the MOLAR heat of combustion of methane(CH₄) if 64.00g of methane are burned to heat 75.0 ml of water from 25.00°C to 95

melamori03 [73]

Answer:

-5.51 kJ/mol

Explanation:

Step 1: Calculate the heat required to heat the water.

We use the following expression.

$Q = c \times m \times \Delta T$

where,

c: specific heat capacity
m: mass
ΔT: change in the temperature

The average density of water is 1 g/mL, so 75.0 mL ≅ 75.0 g.

$Q = 4.184J/g.\°C \times 75.0g \times (95.00\°C - 25.00\°C) = 2.20 \times 10^{3} J = 2.20 kJ$

Step 2: Calculate the heat released by the methane

According to the law of conservation of energy, the sum of the heat released by the combustion of methane (Qc) and the heat absorbed by the water (Qw) is zero

Qc + Qw = 0

Qc = -Qw = -22.0 kJ

Step 3: Calculate the molar heat of combustion of methane.

The molar mass of methane is 16.04 g/mol. We use this data to find the molar heat of combustion of methane, considering that 22.0 kJ are released by the combustion of 64.00 g of methane.

$\frac{-22.0kJ}{64.00g} \times \frac{16.04g}{mol} = -5.51 kJ/mol$

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3 years ago