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2 years ago

[H3O+] = 2.9 x 10-10 M ph level

Chemistry

1 answer:

Zinaida [17]2 years ago

5 0

Answer:

9.54

Explanation:

Fr the question given above, the following data were:

Concentration of hydronium ion [H3O⁺] = 2.9x10¯¹⁰ M

pH =?

The pH of the solution can be obtained as follow:

pH = –Log [H3O⁺]

pH = –Log 2.9x10¯¹⁰

pH = 9.54

Thus, the pH level of the solution is 9.54

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How many grams of h2 will be produced if 175g of HCI are allowed to react completely with sodium

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Answer:

4.8 grams of H₂ will be produced if 175g of HCI are allowed to react completely with sodium

Explanation:

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction) you can see that the following amounts in moles of each compound react and are produced:

HCl: 2 moles
Na: 1 mole
NaCl: 2 moles
H₂: 1 mole

You know the following masses of each element:

H: 1 g/mole
Cl: 35.45 g/mole
Na: 23 g/mole

So, the molar mass of each compound participating in the reaction is:

HCl: 1 g/mole + 35.45 g/mole= 36.45 g/mole
Na: 23 g/mole
NaCl: 23 g/mole + 35.45 g/mole= 58.45 g/mole
H₂: 2* 1 g/mole= 2 g/mole

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HCl: 2 moles* 36.45 g/mole= 72.9 g
Na: 1 mole* 23 g/mole= 23 g
NaCl: 2 moles* 58.45 g/mole= 116.9 g
H₂: 1 mole* 2 g/mole= 2 g

So, a rule of three applies as follows: if by stoichiometry, when reacting 72.9 grams of HCl 2 grams of H₂ are formed, when reacting 175 grams of HCl how much mass of H₂ will be formed?

$mass of H_{2} =\frac{175 g of HCl*2g ofH_{2} }{72.9 g of HCl}$

mass of H₂= 4.8 g

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