explain why an aqueous solution of Na2SO4 is neutral while an aqueous solution of Na2CO3 is basic in nature

Chemistry

1 answer:

exis [7]3 years ago

5 0

The latter contains hydroxyl ions when dissolved in water making it basic.

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sasho [114]

I’m pretty sure it would be B

7 0

3 years ago

Read 2 more answers

7. A solution containing 90grams of KNO3 per 100. grams of H2O at

Tomtit [17]

Answer:

(4) concentrated and supersaturated

Explanation:

At 50.°C, 90g of KNO3 lies above the solubility curve [on the Regents Reference Table G]. This indicates that the solution is supersaturated, meaning it contains more solute than will naturally dissolve, and was formed when a saturated solution cooled. Furthermore, the percent concentration of this solution is 90% KNO3 making this solution concentrated. This can be calculated using the formula for mass percent concentration.

Percent Mass = <u>Mass of Solute (g)</u> x 100

Mass of Solution (g)

5 0

3 years ago

The density of magnesium is 1.7/cm3, and the density of iron is 7.9g/cm3. Consider a block of iron with a mass of 819 g. What is

zepelin [54]

The density of magnesium is 1.7/cm3, and the density of iron is 7.9g/cm3. Consider a block of iron with a mass of 819 g. What is the mass of a block of magnesium that has the same volume as the block of iron?

3 0

3 years ago

Given a chemical equation, showing the dissociation of an acid in solution, be able to identify the "acid", the "base", the "con

Karo-lina-s [1.5K]

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

An acid is defined as a substance which looses donates protons and thus forming conjugate base
A base is defined as a substance which accepts protons and thus forming conjugate acid.

$HA+H_2O\rightarrow A^-+H_3O^+$

Suppose acid Ha is getting dissociated in its solution and after dissociation it donates its proton to water molecule and forms conjugate base. Where as water (acting as a base) accepts protons and forms conjugate acid.

HA = Acid

$H_2O$ = Base