Chemistry, 03.07.2019 06:00 SSE4802

When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. the balanced equation for this reaction is a) kh + bacl → kcl + bah b) koh + bacl → kcl + baoh c) 2koh + bacl2 → 2kcl + ba(oh)2 d) koh + bacl2 → kcl2 + baoh

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Answer from: jfoster70

The correct answer to the question is

Option C. 2KOH + BaCl₂ —> 2KCl + Ba(OH)₂

Potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide.

The equation for the reaction can be written as follow:

Potassium hydroxide => KOH

Barium chloride => BaCl₂

Potassium chloride => KCl

Barium hydroxide => Ba(OH)₂

Potassium hydroxide + Barium chloride —> Potassium chloride + Barium hydroxide

KOH + BaCl₂ —> KCl + Ba(OH)₂

The above equation can be balance as follow:

KOH + BaCl₂ —> KCl + Ba(OH)₂

There are 2 atoms of Cl on the left side and 1 atom on the right. It can be balance by writing 2 before KCl as shown below:

KOH + BaCl₂ —> 2KCl + Ba(OH)₂

There are 2 atoms of K on the right side and 1 atom on the left side. It can be balance by writing 2 before KOH as shown below:

2KOH + BaCl₂ —> 2KCl + Ba(OH)₂

Now, the equation is balanced.

Option C. 2KOH + BaCl₂ —> 2KCl + Ba(OH)₂ gives the correct answer to the question.

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Answer from: jaeybird9

c) $2 \; \text{KOH} + \text{BaCl}_2 \to 2 \; \text{KCl} + \text{Ba}(\text{OH})_2$

Explanation

Start by finding the formula for each of the four species.

The question is asking for a chemical equation. What that means that all species in this equation shall be neutral chemical compounds. Charges from ions shall cancel out within each species such that they end up appearing having no electrical charge.

Potassium hydroxide contains

Potassium ions $\text{K}^{+}$ of charge +1, andHydroxide ions $\text{OH}^{-}$ of charge -1.

Each potassium ion pairs with one hydroxide ion for their charge to cancel out. Potassium hydroxide shall therefore have a chemical formula of $\text{KOH}$ .

Barium chloride contains

Barium ions $\text{Ba}^{2+}$ of charge +2, andChloride ions $\text{Cl}^{-}$ of charge -1.

It takes two chloride ions to cancel out the positive charge on a single barium ion. Barium chloride shall therefore have a chemical formula of $\text{Ba}\text{Cl}_{2}$ (note the subscript attached to chlorine.)

Similarly,

Potassium chloride would be written as $\text{KCl}$ , andBarium hydroxide would be written as $\text{Ba}(\text{OH})_2$ .

Hence the NOT YET BALANCED equation for this reaction:

$\text{KOH} + \text{Ba}\text{Cl}_2 \to \text{KCl} + \text{Ba}(\text{OH})_2$ .

Atoms are conserved in chemical processes. The number of atoms of each element on the left hand side of the arrow shall thus equals to that on the right hand side.

Start by assigning a coefficient of one to one of the species. Then assign coefficients to others on both sides of the equation. It might be necessary to multiply all coefficients by a constant to eliminate any fractional coefficients.

Taking potassium hydroxide as an example:

Assuming that one formula unit of potassium hydroxide takes part in this reaction. There would be one potassium atom on the left hand side of the equation, which- by conservation- should also be present on the other side. One formula unit of potassium chloride should thus be found on the product side.

The chloride atom in potassium chloride attributes to 1/2 formula unit of barium chloride on the product side. There are thus 1/2 barium atoms on both sides of the equation. The chemical equation would therefore be:

$\text{KOH} + 1/2 \; \text{BaCl}_2 \to \text{KCl} + 1/2 \; \text{Ba}(\text{OH})_2$

Multiply all coefficients by 2 to eliminate fractions. Hence the BALANCED chemical equation:

$2 \; \text{KOH} + \text{BaCl}_2 \to 2 \; \text{KCl} +\text{Ba}(\text{OH})_2$ .

Answer from: Quest

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Answer from: Quest

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