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sveta [45]
3 years ago
8

To measure the amount of nickel in some industrial waste fluid, an analytical chemist adds sodium hydroxide solution to a sample

of the fluid and collects the solid nickel(II) hydroxide product. When no more is produced, he filters, washes and weighs it, and finds that has been produced. The balanced chemical equation for the reaction is:
Chemistry
1 answer:
Cloud [144]3 years ago
8 0

Answer:

The final balanced equation is

Ni2+ + 2NaOH --> Ni (OH)2 + 2Na+

Explanation:

It is given that sodium hydroxide is added to collect the solid nickel(II) hydroxide product

The empirical equation for this statement is

Ni2+ + NaOH --> Ni (OH)2 + Na+

We will first balance the hydroxide molecule. On the right side there are two OH molecules.

Thus, on the left side we will take 2 sodium hydroxide

Ni2+ + 2NaOH --> Ni (OH)2 + Na+

Now we will balance the sodium ion which are 2 in numbers on the left side and 1 on the right side

Ni2+ + 2NaOH --> Ni (OH)2 + 2Na+

So, the final balanced equation is

Ni2+ + 2NaOH --> Ni (OH)2 + 2Na+

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Answer: 0.771 g of H_2 will be produced

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} Fe=\frac{14.4g}{56g/mol}=0.257moles

The balanced chemical reaction is:

2Fe(s)+6HCl(aq)\rightarrow 2FeCl_3(aq)+3H_2(g)  

According to stoichiometry :

2 moles of Fe produce = 3 moles of H_2

Thus 0.257 moles of Fe will produce=\frac{3}{2}\times 0.257=0.385moles  of H_2  

Mass of H_2=moles\times {\text {Molar mass}}=0.385moles\times 2g/mol=0.771g

Thus 0.771 g of H_2 will be produced

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What is the molarity of a solution containing 23 g of NaCl in 500 mL of solution?
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molarity of a solution means mols per liter.

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What happens to the ionizing rate if the steps of ionizing polyprotic acid increases?
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