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10 days ago

The oh concentration in a 1.0 x10 3 m ba oh 2 solution is

2 answers:

4 0

Ba(OH)2 breaks down as shown in the equation, resulting in Barium ions and hydroxide ions.
Ba(OH)2 = Ba²⁺ + 2 OH⁻
The concentration of Ba²⁺ ions is 1.0 ×10^-3 M
Consequently, the concentration of OH⁻ ions will be 2× 1.0 ×10^-3 = 2.0 × 10^-3 M
Thus; the answer is 2.0 × 10^-3 M

alisha [964]10 days ago

3 0

The ${\text{O}}{{\text{H}}^ - }$ concentration in a $1.0 \times {10^{ - 3}}{\text{ M Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ solution is $\boxed{2.0 \times {{10}^{ - 3}}{\text{ M}}}$ .

Additional Information:

Concentration expresses the quantitative relationship between different components in a solution. Various terms are utilized to describe this concept. Below are some examples.

1. Molarity (M)

2. Mole fraction (X)

3. Molality (m)

4. Parts per million (ppm)

5. Mass percent ((w/w) %)

6. Volume percent ((v/v) %)

7. Parts per billion (ppb)

Molarity is defined as the amount of solute in one liter of solution. It is denoted as M, with the unit being mol/L. The formula for calculating the molarity of a solution is as follows:

${\text{Molarity of solution}} = \dfrac{{{\text{Moles }}\left( {{\text{mol}}} \right){\text{of solute}}}}{{{\text{Volume }}\left( {\text{L}} \right){\text{ of solution}}}}$

${\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ is categorized as a strong base and dissociates into its constituent ions as shown:

${\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}} \rightleftharpoons {\text{B}}{{\text{a}}^{2 + }} + 2{\text{O}}{{\text{H}}^ - }$

This signifies that one mole of ${\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ dissociates into one mole of ${\text{B}}{{\text{a}}^{2 + }}$ ions and two moles of ${\text{O}}{{\text{H}}^ - }$ ions.

Provided Information:

${\text{Concentration of Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}} = 1.0 \times {10^{ - 3}}{\text{ M}}$

Since one mole of ${\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ produces two moles of ${\text{O}}{{\text{H}}^ - }$ ions, the concentration of ${\text{O}}{{\text{H}}^ - }$ ions will be double that of ${\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ and can be calculated as:

$\begin{aligned}{\text{Concentration of O}}{{\text{H}}^ - } &= 2\left( {1.0 \times {{10}^{ - 3}}{\text{ M}}} \right) \\&= 2.0 \times {10^{ - 3}}{\text{ M}}\\\end{aligned}$

Therefore, the concentration of ${\text{O}}{{\text{H}}^ - }$ ions results in $2.0 \times {10^{ - 3}}{\text{ M}}$ .

Further Reading:

Calculating gas volume:
Determining mole quantity of water:

Answer Summary:

Grade: Senior School

Subject: Chemistry

Chapter: Concentration terms

Keywords: concentration, terminology, solutions, molarity, molality, Ba(OH)2, OH-, Ba2+, 1.0*10^-3 M, 2.0*10^-3 M, molarity, moles of solute, volume, mole fraction, ppm, ppb, mass percent, volume percent.

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Respuesta:

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Answer: The Answer is A.

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