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3 years ago

Which of the following is NOT a strong acid or strong base?

Chemistry

1 answer:

Phoenix [80]3 years ago

4 0

Magnesium hydroxide Mg(OH)₂ is a weak base.

Explanation:

Sulfuric acid H₂SO₄ and hydrochloric acid HCl are, both of them, very strong acids.

Sodium hydroxide NaOH and potassium hydroxide KOH are hydroxides of metals from the first group in the periodic table so thy are strong bases.

As you go to the second group in the periodic table, the hydroxides will not dissociate as much as the hydroxides from the first group in the periodic table , so they will be weak bases. This is the case of magnesium hydroxide Mg(OH)₂.

Learn more about:

acid and bases

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Calculate the volume of a 2.0 molar aqueous solution made from 14 miles of K2S

Vilka [71]

Answer:

volume is 7.0 liters

Explanation:

We are given;

Molarity of the aqueous solution as 2.0 M
Moles of the solute, K₂S as 14 moles

We are required to determine the volume of the solution;

We need to know that;

Molarity = Moles ÷ volume

Therefore;

Volume = Moles ÷ Molarity

Thus;

Volume of the solution = 14 moles ÷ 2.0 M

= 7.0 L

Hence, the volume of the molar solution is 7.0 L

5 0

3 years ago

Match each item with the correct statement below.

V125BC [204]

1. LDFs

2. Intermolecular Forces

3. Intramolecular Forces

4. Linear

5. Tetrahedral

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5 0

3 years ago

The concentrated sulfuric acid we use in the laboratory is 98.0% sulfuric acid by weight. Calculate the molality and molarity of

timama [110]

Answer : The molarity and molality of the solution is, 18.29 mole/L and 499.59 mole/Kg respectively.

Solution : Given,

Density of solution = $1.83g/cm^3=1.83g/ml$

Molar mass of sulfuric acid (solute) = 98.079 g/mole

98.0 % sulfuric acid by mass means that 98.0 gram of sulfuric acid is present in 100 g of solution.

Mass of sulfuric acid (solute) = 98.0 g

Mass of solution = 100 g

Mass of solvent = Mass of solution - Mass of solute = 100 - 98.0 = 2 g

First we have to calculate the volume of solution.

$\text{Volume of solution}=\frac{\text{Mass of solution}}{\text{Density of solution}}=\frac{100g}{1.83g/ml}=54.64ml$

Now we have to calculate the molarity of solution.

$Molarity=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{volume of solution}}=\frac{98.0g\times 1000}{98.079g/mole\times 54.64ml}=18.29mole/L$

Now we have to calculate the molality of the solution.

$Molality=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Mass of solvent}}=\frac{98.0g\times 1000}{98.079g/mole\times 2g}=499.59mole/Kg$

Therefore, the molarity and molality of the solution is, 18.29 mole/L and 499.59 mole/Kg respectively.

7 0

3 years ago

6. What is the molecular formula for this compound? The compound's empirical formula and

igomit [66]

Explanation:

A compound's empirical formula tells you the smallest whole number ratio ,The molar mass tells you what the total mass of one mole

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2 years ago

Please help me

klio [65]

Answer:

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Explanation:

I got it right at school and hope this helps you learn to STUDY.jk

6 0

3 years ago