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timurjin [86]
3 years ago
14

What is the pH of a solution with a concentration of 3.6 × 10-5 molar H3O+? Show, or explain, the work used to solve this proble

m.
Chemistry
2 answers:
Luden [163]3 years ago
7 0

Answer:

pH = 4.45

Explanation:

pH is negative logarithm of the hydrogen ion concentration.  

Given, hydronium ion concentration = 3.6 x 10⁻⁵

pH = - log[H₃O⁺] = - log(3.6 x 10⁻⁵) = 4.45

A pH below 7.0 means the solution is acidic. Neutral pH is at 7.0. For pH above 7.0 the solution is basic.  

lora16 [44]3 years ago
6 0

Answer:

pH = 4.44

Explanation:

You take the negative logarithm of the hydronium ion concentration.

pH = -log[H₃O⁺] = -log(3.6 × 10⁻⁵) = 4.44


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SIZIF [17.4K]

Answer: 0.9375 g

Explanation:

To calculate the number of moles for given molarity, we use the equation:

\text{Moles of solute}={\text{Molarity of the solution}}\times{\text{Volume of solution (in L)}}     .....(1)

Molarity of HCl solution = 0.75 M

Volume of HCl solution = 25.0 mL = 0.025 L

Putting values in equation 1, we get:

\text{Moles of} HCl={0.75}\times{0.025}=0.01875moles  

CaCO_3(s)+2HCl(aq)\rightarrow CaCl_2(s)+CO_2(g)+H_2O(l)  

According to stoichiometry :

2 moles of HCl require = 1 mole of CaCO_3

Thus 0.01875 moles of HCl will require=\frac{1}{2}\times 0.01875=0.009375moles  of CaCO_3

Mass of CaCO_3=moles\times {\text {Molar mass}}=0.009375moles\times 100g/mol=0.9375g

Thus 0.9375 g of CaCO_3 is required to react with 25.0 ml of 0.75 M HCl

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2 years ago
The first step in coal formation process is the formation of:
Reil [10]
Do you have a picture of where you go this question from?
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This volcanic rock formed _____ from lava _____ in gas.
Evgen [1.6K]
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If you burn 55.6 g of hydrogen and produce 497 g of water, how much oxygen reacted?
tester [92]

Answer:

441.28 g Oxygen

Explanation:

  • The combustion of hydrogen gives water as the product.
  • The equation for the reaction is;

2H₂(g) + O₂(g) → 2H₂O(l)

Mass of hydrogen = 55.6 g

Number of moles of hydrogen

Moles = Mass/Molar mass

          = 55.6 g ÷ 2.016 g/mol

          = 27.8 moles

The mole ratio of Hydrogen to Oxygen is 2:1

Therefore;

Number of moles of oxygen = 27.5794 moles ÷ 2

                                               = 13.790 moles

Mass of oxygen gas will therefore be;

Mass = Number of moles × Molar mass

Molar mass of oxygen gas is 32 g/mol

Mass = 13.790 moles × 32 g/mol

<h3>          = 441.28 g</h3><h3>Alternatively:</h3>

Mass of hydrogen + mass of oxygen = Mass of water

Therefore;

Mass of oxygen = Mass of water - mass of hydrogen

                          = 497 g - 55.6 g

<h3>                           = 441.4 g </h3>
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Answer:

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Explanation:

Hydrogen can never be central atom despite its low electronegativity

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