What is an example of a strong base? HCl NaCl NaOH HF

Calculate the molar solubility of pbi2 in the presence of 0.10 m nai.

lys-0071 [83]

The equation representing the solubility of $PbI_{2}$ :

$PbI_{2}(aq)Pb^{2+}(aq) + 2 I^{-}(aq)$

5 0

3 years ago

what is the substances would be produced during the chemical reaction between potassium hydroxide and hydrochloric acid

tino4ka555 [31]

Potassium chloride and water

3 0

4 years ago

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How many grams of S are in 665 g of SO2

ollegr [7]

Answer: 111g S

Explanation:

SO2 you have = 665 g

SO2 molar mass = 64.066 g/mol

S molar mass = 32.065 g/mol

$665g SO2*\frac{1 molSO2}{64.066gSO2} *\frac{1molS}{3molSO2} * \frac{32.065gS}{1molS} = 110.944... ~ 111gS$

4 0

3 years ago

What is the oxidation state Ca(NO3)2

mylen [45]

Oxidation state is a number that is assigned to an element in a chemical combination. The number represents the number of electrons that an atom can gain, loses, or share when chemically bonding with an atom of another element. In this case the oxidation state or the oxidation number of Ca(NO3)2 is Zero, since its an electrically neutral compound. Thus the sum of oxidation number of calcium, nitrogen and oxygen is zero.

8 0

3 years ago

An iron storage tank is placed in the ocean with no cathodic protection. a. What is the electrolyte in this reaction? b. As the

MariettaO [177]

Answer:

Iron is being oxidized at the anode and water is acting as the electrolyte.

Explanation:

When iron is exposed to oxygen and water , the rusting of iron takes place.

The reaction taking place at anode : Oxidation of iron.

${anode:}\;\text{Fe}(s)\;{\longrightarrow}\;\text{Fe}^{2+}(aq)\;+\;2\text{e}^{-}$

The reaction taking place at cathode : Reduction of oxygen in the air.

${cathode:}\;\text{O}_2(g)\;+\;4\text{H}^{+}(aq)\;+\;4\text{e}^{-}\;{\longrightarrow}\;2\text{H}_2\text{O}(l)$

The overall reaction:

${overall:}\;2\text{Fe}(s)\;+\;\text{O}_2(g)\;+\;4\text{H}^{+}(aq)\;{\longrightarrow}\;2\text{Fe}^{2+}(aq)\;+\;2\text{H}_2\text{O}(l)$

The rust that is hydrated iron(III) oxide can form iron(II) ions which can react further with oxygen.

$4\text{Fe}^{2+}(aq)\;+\;\text{O}_2(g)\;+\;(4\;+\;2x)\;\text{H}_2\text{O}(l)\;{\longrightarrow}\;2\text{Fe}_2\text{O}_3{\cdot}x\text{H}_2\text{O}(s)\;+\;8\text{H}^{+}(aq)$

Thus, from the above reactions ,

Iron is being oxidized at the anode and water is acting as the electrolyte.

3 0

4 years ago