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4 years ago

K2so4 is a strong electrolyte. determine the concentration of each of the individual ions in a 0.600 m k2so4 solution.

1 answer:

6 0

Potassium sulfate or K₂SO₄ is a strong electrolyte which means that it will completely dissociate into ions when dissolved in water. The dissociation reaction is as follows:

K₂SO₄ → 2K⁺ + SO₄²⁻

This means that the dissociation of 1 mol of K₂SO₄ solution will yield 2 moles of K⁺ and 1 mole of SO₄²⁻. Molarity is a measure of concentration defined as moles divided by the volume of solution. In this case, given that the volume is constant, from stoichiometry, the concentration of K⁺ ions would be twice of 0.600 M which is 1.200 M. On the other hand, the concentration of SO₄²⁻ is 0.600 M by stoichiometry.

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Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below. 2HgO Rig

yulyashka [42]

15.63 moles of HgO are needed to produce 250. 0 grams of Oxygen.

<h3>How we calculate moles from masses?</h3>

Moles of any substance can be calculated as:

n =W/M, where

W = given mass

M = molar mass

Given chemical reaction is:

2HgO → 2Hg + O₂

From the stoichiometry of the reaction, it is clear that:

2 mole of HgO = produce 1 mole of O₂

Given mass of O₂ = 250 grams

Molar mass of O₂ = 32 g/mole

Mole of produced O₂ = 250g / 32g/mole = 7.81 moles

Now, 7.81 moles of O₂ = produced by 2×7.81 = 15.63 moles of HgO

Hence, option (3) is correct i.e. 15.63 moles is the required moles.

To know more about moles, visit the below link:

brainly.com/question/16060223

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3 years ago

Aspirin is well known as a pain reliever (analgesic) and as a fever reducer (antipyretic). It has a molar mass of 180.2 g/mol an

denis23 [38]

Answer: The molecular formula of aspirin is $C_8H_8O_2$

Explanation:

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of C= 60.0 g

Mass of H = 4.5 g

Mass of O = 35.5 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{60.0g}{12g/mole}=5.00moles$

Moles of H = $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{4.5g}{1g/mole}=4.5moles$

Moles of O = $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{35.5g}{16g/mole}=2.22moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{5.00}{2.22}=2$

For H = $\frac{4.5}{2.22}=2$

For O = $\frac{2.22}{2.22}=1$

The ratio of C : H: O= 2: 2: 1

Hence the empirical formula is $C_2H_2O$

The empirical weight of $C_2H_2O$ = 2(12)+2(1)+1(16)= 42g.

The molecular weight = 180.2 g/mole

Now we have to calculate the molecular formula.

$n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{180.2}{42}=4$

The molecular formula will be= $4\times C_2H_2O=C_8H_8O_2$

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