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-Dominant- [34]
2 years ago
7

For Mn3+, write an equation that shows how the cation acts as an acid.

Chemistry
2 answers:
Mkey [24]2 years ago
8 0

An acid is a compound which will give H+ ions or H3O^+  ions

the reaction will be

[Mn(H_{2}O )_{6} ^{+3} +H_{2}O --> [MnOH(H_{2}O)_{5}]^{+2} + H_{3}O^{+}

Thus as there is evolution of H_{3}O^{+} the Mn+3 is an acid

yuradex [85]2 years ago
7 0

The equation that shows {\text{M}}{{\text{n}}^{3 + }}  acts as the acid is

\boxed{{{\left[{{\text{Mn}}{{\left({{{\text{H}}_2}{\text{O}}}\right)}_6}}\right]}^{3 + }}+{{\text{H}}_2}{\text{O}}\to{{\left[ {{\text{MnOH}}{{\left({{{\text{H}}_2}{\text{O}}} \right)}_5}}\right]}^{2 + }}{{\text{H}}_3}{{\text{O}}^ + }}

Further Explanation:

Acids and bases can be defined in many ways based on different theories, which are as follows:

1. Arrhenius theory: According to this theory, acid is defined as the one which produces hydrogen or hydronium ions in a solution, while the base is defined as the one which produces hydroxide ions in a solution. Examples of Arrhenius acids include HBr, {\text{HN}}{{\text{O}}_3} and  {{\text{H}}_2}{\text{S}}{{\text{O}}_4} while NaOH and KOH are examples of Arrhenius bases.

2. Bronsted-Lowry theory: According to this theory, the acid in the reaction donates a proton while a base is one that accepts a proton. HCl acts as Bronsted acid while {\text{N}}{{\text{H}}_3} is a Bronsted base.

3. Lewis theory: According to this theory, an acid accepts a pair of electrons to electron-rich species while a base donates electrons to electron-deficient species in the reaction. Examples of Lewis acids are {\text{B}}{{\text{F}}_3} , {\text{S}}{{\text{O}}_3} while {{\text{H}}_2}{\text{O}} and ROH are the examples of Lewis base.

The equation to show the acidic nature of {\mathbf{M}}{{\mathbf{n}}^{{\mathbf{3 + }}}} is as follows:

{\left[ {{\text{Mn}}{{\left({{{\text{H}}_2}{\text{O}}}\right)}_6}}\right]^{3 + }}+{{\text{H}}_2}{\text{O}}\to {\left[{{\text{MnOH}}{{\left( {{{\text{H}}_2}{\text{O}}}\right)}_5}} \right]^{2+}}+{{\text{H}}_3}{{\text{O}}^+}

Here, {\text{M}}{{\text{n}}^{3 + }} exists as {\left[{{\text{Mn}}{{\left( {{{\text{H}}_2}{\text{O}}}\right)}_6}}\right]^{3 + }} in the aqueous medium. It reacts with water molecule to form {\left[{{\mathbf{MnOH}}{{\left( {{{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}} \right)}_{\mathbf{5}}}} \right]^{{\mathbf{2 + }}}} and {{\mathbf{H}}_{\mathbf{3}}}{{\mathbf{O}}^{\mathbf{ + }}} is also released during the reaction.

Learn more:

1. The reason for the acidity of water brainly.com/question/1550328

2. Reason for the acidic and basic nature of amino acid brainly.com/question/5050077

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: acid, Mn3+, Arrhenius theory, Bronsted-Lowry theory, Lewis theory, H3O+, HCl, NH3, BF3, SO3, hydrogen ions, hydronium ions, hydroxide ions, aqueous, water, Mn(H20)63+, MnOH(H2O)63+, H2O, accepts, donates, electrons, reaction, proton.

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Data:
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Solving:

1 mole of arsenic → 75g ------------ 6,02*10²³ molecules
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6,02*10²³X = 75
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2 years ago
Which of the following is an example of a Lewis acid?
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Answer:

C. BF3

Explanation:

The boron in BF3 is electron poor and has an empty orbital, so it can accept a pair of electrons, making it a Lewis acid.

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4 0
2 years ago
How many kilograms of solvent would contain 0.43 mol of CaO in a 2.5 molality solution
dalvyx [7]
<h3>Answer:</h3>

0.024 kg CaO

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

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Aqueous Solutions</u>

  • Molarity = moles of solute / liters of solution

<u>Atomic Structure</u>

  • Reading a Periodic Tables
  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

0.41 mol CaO

2.5 M Solution

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

1000 g = 1 kg

Molar Mass of Ca - 40.08 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of CaO - 40.08 + 16.00 = 56.08 g/mol

<u>Step 3: Convert</u>

  1. Set up:                                \displaystyle 0.43 \ mol \ CaO(\frac{56.08 \ g \ Cao}{1 \ mol \ CaO})(\frac{1 \ kg \ CaO}{1000 \ g \ CaO})
  2. Multiply:                              \displaystyle 0.024114 \ kg \ CaO

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs as our lowest.</em>

0.024114 kg CaO ≈ 0.024 kg CaO

4 0
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