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1 year ago

What is the ph of an aqueous solution with a hydrogen ion concentration of [H+]=1. 2×10^−8 m?

Chemistry

1 answer:

il63 [147K]1 year ago

4 0

The pH of an aqueous solution with a hydrogen ion concentration of [H+]=1. 2×10^−8 m is 7.92.

The entire form of pH is potential of Hydrogen. pH is called the poor logarithm of H+ ion attention. hence the that means of the name pH is explained because the energy of hydrogen. pH describes the concentration of the hydrogen ions in a solution and it's miles the indicator of acidity or basicity.

pH is an important amount that reflects the chemical conditions of an answer. The pH can manage the provision of vitamins, organic features, microbial activity, and the conduct of chemical substances.

pH stands for capacity hydrogen and it's used to explain the acidity or alkalinity of a substance. The pH scale is measured from 1 to fourteen. 7 is impartial and the lower the quantity, the extra acidic and the higher, the greater alkaline.

explaination,

[H+]=1. 2×10^−8 m

log[h+] = 1. 2×10^−8 m

= 8 - log (1.2)

= 8 - 0.079

PH = 7.921

Learn more about pH here:-brainly.com/question/172153

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Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the f

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Explanation:

As per Brønsted-Lowry concept of acids and bases, chemical species which donate proton are called Brønsted-Lowry acids.

The chemical species which accept proton are called Brønsted-Lowry base.

(a) $HNO_3 + H_2O \rightarrow H_3O^+ + NO_3^-$

$HNO_3$ is Bronsted lowry acid and $NO_3^-$ is its conjugate base.

$H_2O$ is Bronsted lowry base and $H_3O^+$ is its conjugate acid.

(b)

$CN^- + H_2O \rightarrow HCN + OH^-$

$CN^-$ is Bronsted lowry base and HCN is its conjugate acid.

$H_2O$ is Bronsted lowry acid and $OH^-$ is its conjugate base.

(c)

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$H_2SO_4$ is Bronsted lowry acid and $HSO_4^-$ is its conjugate base.

Cl^- is Bronsted lowry base and HCl is its conjugate acid.

(d)

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$HSO_4^-$ is Bronsted lowry acid and $SO_4^{2-}$ is its conjugate base.

OH^- is Bronsted lowry base and $H_2O$ is its conjugate acid.

(e)

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3 years ago

How much water (H2O ) would form if 4.04 g of hydrogen (H2) reacted with 31.98 g of oxygen (O2 )?

Norma-Jean [14]

Answer:

Mass = 36 g

Explanation:

Given data:

Mass of water formed = ?

Mass of hydrogen = 4.04 g

Mass of oxygen = 31.98 g

Solution:

Chemical equation:

2H₂ + O₂ → 2H₂O

Number of moles of hydrogen:

Number of moles = mass/molar mass

Number of moles = 4.04 g/ 2 g/mol

Number of moles = 2.02 mol

Number of moles of oxygen:

Number of moles = mass/molar mass

Number of moles = 31.98 g/ 32 g/mol

Number of moles = 1.0 mol

Now we will compare the moles of water with hydrogen and oxygen.

O₂ : H₂O

1 : 2

H₂ : H₂O

2 : 2

2.02 : 2.02

Number of moles of water formed by oxygen are less thus oxygen will limiting reactant.

Mass of water:

Mass = number of moles × molar mass

Mass = 2 mol × 18 g/mol

Mass = 36 g

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