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2 years ago

8

In its aqueous solution, 99.9% of a substance dissociates to release hydronium ions. Which of the following is true for the subs

tance? (3 points)
a
It is a weak acid.

b
It is a weak base.

c
It is a strong acid.

d
It is a strong base.

2 answers:

lesantik [10]2 years ago

5 0

Answer:

C

Explanation:

It is a strong acid.

(Took the test!)

olga2289 [7]2 years ago

3 0

The answer is C. It’s a strong acid

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If there are 0.2 M solutions of both acid and base, the concentrations of hydrogen and hydroxide ions will be equal at equivalence point.

The reaction of sulfuric acid and a basic solution BOH occurs as follows;

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In the question, we are told that that both the solution of the sulfuric acid and the basic solution are 0.2 M.

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Following the instructions in your lab manual, you have titrated a 25.00 mL sample of 0.0100 M KIO3 with a solution of Na2S2O3 o

vivado [14]

<u>Answer:</u>

<u>For 1:</u> The amount of potassium iodate that were titrated is $2.5\times 10^{-4}$ moles

<u>For 2:</u> The amount of sodium thiosulfate required is $1.25\times 10^{-4}$ moles

<u>Explanation:</u>

<u>For 1:</u>

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in L)}}$

Molarity of $KIO_3$ solution = 0.0100 M

Volume of solution = 25 mL

Putting values in above equation, we get:

$0.0100M=\frac{\text{Moles of }KIO_3\times 1000}{25}\\\\\text{Moles of }KIO_3=\frac{0.0100\times 25}{1000}=0.00025mol$

Hence, the amount of potassium iodate that were titrated is $2.5\times 10^{-4}$ moles

<u>For 2:</u>

The chemical equation for the reaction of potassium iodate and sodium thiosulfate follows:

$2KIO_3+Na_2S_2O_3\rightarrow K_2S_2O_3+2NaIO_3$

By Stoichiometry of the reaction:

2 moles of potassium iodate reacts with 1 mole of sodium thiosulfate

So, 0.00025 moles of potassium iodate will react with = $\frac{1}{2}\times 0.00025=0.000125mol$ of sodium thiosulfate

Hence, the amount of sodium thiosulfate required is $1.25\times 10^{-4}$ moles

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3 years ago

In order to predict the outcome of the reaction, write the molecular, full ionic, and net ionic equations for a mixture of aqueo

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Answer:

See explanation

Explanation:

Full molecular equation;

2NH3(aq) + AgNO3(aq) -------> [Ag(NH3)2]NO3(aq)

Full ionic equation

2NH3(aq) + Ag^+(aq) + NO3^-(aq) --------> [Ag(NH3)2]^+(aq) + NO3^-(aq)

Net ionic equation;

2NH3(aq) + Ag^+(aq) --------> [Ag(NH3)2]^+(aq)

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Magnesium reacts with sulfuric acid in an exothermique reaction. Write an equation for the reaction. Include state symbols in yo

goldenfox [79]

Answer:

The reaction between magnesium and sulphuric acid is given as :

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Explanation:

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2 years ago