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4 years ago

Why do weak acid-weak base reactions not go to completion?

Chemistry

2 answers:

dezoksy [38]4 years ago

7 0

Answer: Option (c) is the correct answer.

Explanation:

Weak acid and weak bases are the species that dissociate weakly in a solvent or water.

For example, acetic acid ( $CH_{3}COOH$ ) is a weak acid and it dissociates poorly in water.

Hence, we can say that due to weak dissociation there will less formation of hydrogen or hydroxide ions upon dissociation of weak acid or weak base. Therefore, due to lack of sufficient number of ions the reaction will not go to completion.

Thus, we can conclude that weak acid-weak base reactions not go to completion because neither a weak acid nor a weak base has a strong tendency to transfer $H^+$ ions.

vladimir2022 [97]4 years ago

4 0

Neither a weak acid nor a weak base has a strong tendency to transfer H+ ions that is why<span> weak acid-weak base reactions not go to completion.</span>

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3 years ago

How many grams of copper would have the same number of atoms as 139.82 grams of argon

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3 years ago

What are the characteristics of an atom or molecule when in the gas phase

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Answer:vapor

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3 years ago

Read 2 more answers

Samples of three different compounds were analyzed and the masses of each element were determined.

Dafna1 [17]

First, you have to convert mass to moles by making use of molecular weights [N = 14 g/mol and O = 16 g/mol)

A.
5.6/14 = 0.4 mol N
3.2/16 = 0.2 mol O
mol ratio = 2 mol N/1 mol O => N2O

B.
3.5/14 = 0.25 mol N
8.0/16 = 0.5 mol O
mol ratio = 1 mol N/2 mol O => NO2

C.
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3 years ago

The equations are 2NaHCO3 -> Na2CO3 + CO2 + H20, NaHCO3 -> NaOH + CO2, 2NaHCO3 -> Na2O + 2CO2 + H20

cricket20 [7]

Answer:

The product made is Na2CO3.

The % yield is 91.8 %

Explanation:

Step 1: Data given

Mass of baking soda (NaHCO3) = 5.0 grams

Molar mass of NaHCO3 = 84.0 g/mol

Each of the equations calculated is left with 2.4g of NaOH, 1.86 g Na2O, and 3.18g Na2Co3.

Step 2: The balanced equations

2NaHCO3 → Na2CO3 + CO2 + H20

NaHCO3 → NaOH + CO2

2NaHCO3 → Na2O + 2CO2 + H20

Step 3: Calculate moles NaHCO3

Moles NaHCO3 = mass NaHCO3 / molar mass NaHCO3

Moles NaHCO3 = 5.0 grams / 84.0 g/mol

Moles NaHCO3 = 0.060 moles

Step 4: Calculate moles of products

For 2 moles NaHCO3 we'll have 1 mol Na2CO3

For 0.060 moles NaHCO3 we'lll have 0.060 / 2 = 0.030 moles Na2CO3

For 1 mol NaHCO3 we'll have 1 mol NaOH

For 0.060 moles NaHCO3 we'll have 0.060 moles NaOH

For 2 moles NaHCO3 we'll have 1 mol Na2O

For 0.060 moles NaHCO3 we'll have 0.030 moles Na2O

Step 5: Calculate mass of products

Mass = moles * molar mass

Mass of Na2CO3 = 0.030 moles * 105.99 g/mol = 3.18 grams

Mass of NaOH = 0.060 moles * 40.0 g/mol = 2.4 grams

Mass of Na2O = 0.030 moles *61.98 g/mol = 1.86 grams

Step 6: Calculate the percent yield

% yield = actual yield / theoretical yield

% yield Na2CO3 = (2.92 grams / 3.18 grams) *100% = 91.8 %

% yield NaOH = (2.92 grams / 2.4 grams ) *100% = 121.6 %

% yield of Na2O = (2.92 grams / 1.86 grams ) * 100% = 157 %

The product made is Na2CO3, the other reactions have a % yield greater than 100 %

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3 years ago