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3 years ago

Acid formulas can be distinguished from base formulas because acid formulas usually and base formulas .

Chemistry

1 answer:

sineoko [7]3 years ago

3 0

Answer:

A. begin with hydrogen; pair a metal with a hydroxide ion

Explanation:

Acid can be distinguished from base on the basis of formulas in such a way that acid formula start with hydrogen.

For example:

Hydrochloric acid is strong acid. Its formula is HCl.

It start with hydrogen

Sulfuric acid is acid. Its formula is H₂SO₄

it is also start with hydrogen.

Base:

Base is distinguish from acid in such a way that in base formula metal is pair with hydroxide ion.

For example:

Sodium hydroxide is base. Its formula is NaOH.

sodium is metal while OH is hydroxide ion.

Potassium hydroxide is base. its formula is KOH.

potassium is metal and OH is hydroxide ion.

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How is Hess's law used to measure enthalpy of a desired reaction?

Morgarella [4.7K]

Answer:

Explanation:

I hope this is correct

6 0

3 years ago

Determine the acid dissociation constant for a 0.020 m formic acid solution that has a ph of 2.74. formic acid is a weak monopro

Setler [38]

Answer:

Ka = 1.82x10⁻⁴

Explanation:

To solve this problem, we need a basis. In this case, we need the overall reaction and a ICE chart. So, let's write the overall reaction first:

HCOOH + H₂O <--------> H₃O⁺ + HCOO⁻ Ka = ?

Now that we have the overall reaction, we need to write the ICE chart. In this way we can determine what data do we have, and what do we have left to determine:

HCOOH + H₂O <--------> H₃O⁺ + HCOO⁻ Ka = ?

i) 0.02 0 0

e) 0.02-x x x

The Ka expression is:

Ka = [H₃O⁺] [HCOO⁻] / [HCOOH]

Replacing the given data we have:

Ka = x² / 0.02 - x

Now, the value of x can be calculated because we already have the pH of the formic acid, and with it, we can calculate the [H₃O⁺] with the following expression:

[H₃O⁺] = 10^(-pH)

Replacing we have:

[H₃O⁺] = 10^(-2.74) = 1.82x10⁻³ M

This is the value of x, so replacing in the Ka expression, we can calculate then, the value of Ka:

Ka = (1.82x10⁻³)² / (0.02 - 1.82x10⁻³)

7 0

3 years ago

An aqueous solution of acetic acid is found to have the following equilibrium concentrations at 25 C:

yarga [219]

Answer: 1.79 x 10^-5

Explanation: The equilibrium constant of a reaction can be calculated from the quotient of the concentrations of the products over the concentrations of the reactants, with each termed raised to their respective stoichometric coefficients.

For acetic acid, this equilibrium expression is:

$Kc=\frac{[H+] [CH3COO-]}{[CH3COOH]}$

Replacing the equilibrium concentrations given by the exercise into the expression above, the equilibrium constant, Kc will be obtained and it is found to be equal to 1.79 x 10^-5.