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Harlamova29_29 [7]
3 years ago
5

Determine whether or not each ion contributes to water hardness.

Chemistry
1 answer:
Virty [35]3 years ago
4 0

Answer: The ion that contribute to water hardness are:

--> a. Ca2+

--> b. (HCO)3^- and

--> c. Mg2+

While K+ DOES NOT contribute to water hardness.

Explanation:

WATER in chemistry is known as a universal solvent. This is so because it is polar in nature and dissolves most inorganic solutes and some polar organic solutes to form aqueous solutions. It is composed of elements such as hydrogen and oxygen in the combined ratio of 2:1.

Water is said to be HARD if it does not lather readily with soap. There are two types of water hardness:

--> Permanent hardness: This is mainly due to the presence of CALCIUM and MAGNESIUM ions in the form of soluble tetraoxosulphate(VI) and chlorides. These ions are removed by adding washing soda or caustic soda.

--> Temporary hardness: This is due to the presence of calcium HYDROGENTRIOXOCARBONATES. It can be removed by boiling and using slaked lime.

Therefore from the above given ions, Ca2+,(HCO)3^- and Mg2+ contributes to water hardness.

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Microbe

Explanation:

It can be microbe or microorganisms.

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Answer:

The answer is the explanation.

Explanation:

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2CH3COOH + Ca(OH)2 → 2CH3COO- + 2H2O + Ca²⁺

That means the moles of acetic acid decrease whereas the moles of  acetate ion are increased. The ratio of [CH3COOH] / [CH3COO-] is different.

As a base is added, the concentration of H3O+ decreases increasing the pH.

That means:

<em>TRUE </em> A. The number of moles of CH3COOH will decrease.

<em>FALSE</em> B. The number of moles of CH3COO- will decrease.

<em>TRUE </em>C. The equilibrium concentration of H3O will decrease.

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AgNO3(aq)+Na3PO4(aq) ionic equation
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All species are "(aq)" unless marked otherwise:

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total ionic: 3 Na{+} + PO4{3-} + 3 Ag{+} + 3 NO3{-} → Ag3PO4(s) + 3 Na{+} + 3 NO3{-}
net ionic: PO4{3-} + 3 Ag{+} → Ag3PO4(s)

K2SO4(aq)+Na2CO3(aq) no reaction

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total ionic: Pb{2+} + 2 NO3{-} + 2 Na{+} + CO3{2-} → PbCO3(s) + 2 Na{+} + 2 NO3{-}
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molecular: BaCl2 + 2 KOH → Ba(OH)2(s) + 2 KCl
total ionic: Ba{2+} + 2 Cl{-} + 2 K{+} + 2 OH{-} → Ba(OH)2(s) + 2 K{+} + 2 Cl{-}
net ionic: Ba{2+} + 2 OH{-} → Ba(OH)2(s)
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3 years ago
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