Math / Algebra

QuestionWhich of the following is the correct expression for the $K_{s p}$ of $\mathrm{MgCO}_{3}$ ? $\mathrm{K}_{\mathrm{sp}}=\left[\mathrm{Mg}^{2+}\right]\left[\mathrm{CO}_{3}^{2-}\right]$ $\mathrm{K}_{\mathrm{sp}}=\frac{1}{\left[\mathrm{Mg}^{2+} \mid\left[\mathrm{CO}_{3}^{2}\right]\right.}$ $\mathbb{K}_{\text {sp }}=\left[\mathrm{Mg}^{2+}\right]\left[\mathrm{CO}^{2-}\right]^{3}$ $\mathbb{K}_{\text {sp }}=\frac{\left[60_{-1}^{2}\right]}{\left[\mathrm{Mg}^{2+1}\right]}$ $\left.\mathrm{x}_{s p}=\left[\mathrm{Mg}^{2+}\right][C]\left[\mathrm{O}_{3}^{2-}\right]\right]$

Studdy Solution

STEP 1

What is this asking? Which expression correctly shows how much magnesium carbonate dissolves in a solution? Watch out! Don't mix up the K_sp expression with other equilibrium expressions! K_sp is specifically for how much a solid dissolves.

STEP 2

1. Understand K_sp
2. Write the balanced dissolution equation
3. Build the K_sp expression

STEP 3

K_sp, the solubility product constant, tells us how much a solid dissolves into its ions in a saturated solution.
A bigger K_sp means more dissolving!
It's like a popularity contest for dissolved ions!

STEP 4

K_sp is all about equilibrium.
When the solid is dissolving as fast as the ions are coming back together, we've hit equilibrium, and K_sp describes that balance.

STEP 5

We're dealing with magnesium carbonate, MgCO₃ $_{(s)}$ .
When it dissolves, it breaks into its ions: magnesium, Mg²⁺ $_{(aq)}$ , and carbonate, CO₃²⁻ $_{(aq)}$ .

STEP 6

The balanced equation looks like this: $\text{MgCO}_3(s) \rightleftharpoons \text{Mg}^{2+}(aq) + \text{CO}_3^{2-}(aq)$ See? One magnesium carbonate breaks down into one magnesium ion and one carbonate ion.
Perfectly balanced, as all things should be!

STEP 7

The K_sp expression is built by multiplying the concentrations of the dissolved ions, each raised to the power of its coefficient in the balanced equation.

STEP 8

From our balanced equation, both Mg²⁺ and CO₃²⁻ have a coefficient of 1.
So, our K_sp expression is: $K_{sp} = [\text{Mg}^{2+}]^1 \cdot [\text{CO}_3^{2-}]^1$ We don't include the solid MgCO₃ $_{(s)}$ in the K_sp expression because its concentration is constant.

STEP 9

Since anything raised to the power of 1 is just itself, we can simplify to: $K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}]$

STEP 10

The correct expression for the K_sp of MgCO₃ is $K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}]$ , which is the first option.

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Studdy Solution

STEP 1

What is this asking? Which expression correctly shows how much magnesium carbonate dissolves in a solution? Watch out! Don't mix up the K_sp expression with other equilibrium expressions! K_sp is specifically for how much a solid dissolves.

STEP 2

1. Understand K_sp
2. Write the balanced dissolution equation
3. Build the K_sp expression

STEP 3

K_sp, the solubility product constant, tells us how much a solid dissolves into its ions in a saturated solution.
A bigger K_sp means more dissolving!
It's like a popularity contest for dissolved ions!

STEP 4

K_sp is all about equilibrium.
When the solid is dissolving as fast as the ions are coming back together, we've hit equilibrium, and K_sp describes that balance.

STEP 5

We're dealing with magnesium carbonate, MgCO₃ $_{(s)}$ .
When it dissolves, it breaks into its ions: magnesium, Mg²⁺ $_{(aq)}$ , and carbonate, CO₃²⁻ $_{(aq)}$ .

STEP 6

The balanced equation looks like this: $\text{MgCO}_3(s) \rightleftharpoons \text{Mg}^{2+}(aq) + \text{CO}_3^{2-}(aq)$ See? One magnesium carbonate breaks down into one magnesium ion and one carbonate ion.
Perfectly balanced, as all things should be!

STEP 7

The K_sp expression is built by multiplying the concentrations of the dissolved ions, each raised to the power of its coefficient in the balanced equation.

STEP 8

From our balanced equation, both Mg²⁺ and CO₃²⁻ have a coefficient of 1.
So, our K_sp expression is: $K_{sp} = [\text{Mg}^{2+}]^1 \cdot [\text{CO}_3^{2-}]^1$ We don't include the solid MgCO₃ $_{(s)}$ in the K_sp expression because its concentration is constant.

STEP 9

Since anything raised to the power of 1 is just itself, we can simplify to: $K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}]$

STEP 10

The correct expression for the K_sp of MgCO₃ is $K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}]$ , which is the first option.

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Studdy Solution

STEP 1

What is this asking? Which expression correctly shows how much magnesium carbonate dissolves in a solution? Watch out! Don't mix up the *K*sp expression with other equilibrium expressions! *K*sp is specifically for how much a solid dissolves.

STEP 2

1. Understand *K*sp2. Write the balanced dissolution equation3. Build the *K*sp expression

STEP 3

*K*sp, the **solubility product constant**, tells us how much a solid dissolves into its ions in a saturated solution.A bigger *K*sp means more dissolving!It's like a popularity contest for dissolved ions!

STEP 4

*K*sp is all about **equilibrium**.When the solid is dissolving as fast as the ions are coming back together, we've hit equilibrium, and *K*sp describes that balance.

STEP 5

We're dealing with magnesium carbonate, MgCO3(s)_{(s)}(s)​.When it dissolves, it breaks into its ions: magnesium, Mg2+(aq)_{(aq)}(aq)​, and carbonate, CO32−(aq)_{(aq)}(aq)​.

STEP 6

STEP 7

The *K*sp expression is built by multiplying the concentrations of the dissolved ions, each raised to the power of its coefficient in the balanced equation.

STEP 8

STEP 9

Since anything raised to the power of 1 is just itself, we can simplify to: Ksp=[Mg2+]⋅[CO32−] K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}] Ksp​=[Mg2+]⋅[CO32−​]

STEP 10

The correct expression for the *K*sp of MgCO3 is Ksp=[Mg2+]⋅[CO32−] K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}] Ksp​=[Mg2+]⋅[CO32−​], which is the first option.

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Start learning now

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What is this asking? Which expression correctly shows how much magnesium carbonate dissolves in a solution? Watch out! Don't mix up the K_sp expression with other equilibrium expressions! K_sp is specifically for how much a solid dissolves.

1. Understand K_sp
2. Write the balanced dissolution equation
3. Build the K_sp expression

K_sp, the solubility product constant, tells us how much a solid dissolves into its ions in a saturated solution.
A bigger K_sp means more dissolving!
It's like a popularity contest for dissolved ions!

K_sp is all about equilibrium.
When the solid is dissolving as fast as the ions are coming back together, we've hit equilibrium, and K_sp describes that balance.

We're dealing with magnesium carbonate, MgCO₃ $_{(s)}$ .
When it dissolves, it breaks into its ions: magnesium, Mg²⁺ $_{(aq)}$ , and carbonate, CO₃²⁻ $_{(aq)}$ .

The K_sp expression is built by multiplying the concentrations of the dissolved ions, each raised to the power of its coefficient in the balanced equation.

Since anything raised to the power of 1 is just itself, we can simplify to: $K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}]$

The correct expression for the K_sp of MgCO₃ is $K_{sp} = [\text{Mg}^{2+}] \cdot [\text{CO}_3^{2-}]$ , which is the first option.