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3 years ago

Without doing any calculations, determine which of the following solutions would be most acidic.

Chemistry

1 answer:

Murljashka [212]3 years ago

5 0

Answer:

In the first combination neutralization takes place to give a salt. So, solution 'a' is neutral in nature.

In the solution 'c', both salts are resulted by the combination of weak base and strong acid. The combination of these salts suppresses the acidity.

In last combination basic nature is observed due to the presence of CN⁻ ions. Thus, the solution 'd' is basic in nature.

Out of the five given solutions, 0.0100 M in HF and 0.0100 M in KBr is most acidic. Therefore, solution 'b' is most acidic in nature.

Explanation:

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<h3>Answer:</h3>

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<h3>General Formulas and Concepts:</h3>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

4 mol Co (Cobalt)

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

Set up: $\displaystyle 4 \ mol \ Co(\frac{6.022 \cdot 10^{23} \ atoms \ Co}{1 \ mol \ Co})$
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<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 1 sig fig.</em>

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