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Mama L [17]
3 years ago
6

g An analytical chemist is titrating of a solution of diethylamine with a solution of . The of diethylamine is . Calculate the p

H of the base solution after the chemist has added of the solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of solution added. hno3
Chemistry
1 answer:
Serga [27]3 years ago
5 0

Answer:

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Explanation:

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What is the reason for attainment of equilibrium?
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When a reversible reaction happens in a closed container, it reaches a dynamic equilibrium . At equilibrium: the forward and backward reactions are still happening. the forward and backward reactions have the same rate of reaction

Explanation:

4 0
3 years ago
Most gases exist as molecules, for example, fluorine is F2.
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They are all stable and have eight valence electrons
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Which of the following compound is most soluble in water a)glycerol b) ethyl alcohol c) ethylene glycol d)ethyl chloride
lubasha [3.4K]

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glycerol

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it is thick sweet liquid.It is type of alcohol which has 3 OH groups

4 0
2 years ago
Please help with chemistry homework (I’ll mark brainliest!)
masha68 [24]

Answer:

You answer is correct

Electrons have a negative charge. The charge on the proton and electron are exactly the same size but opposite. Neutrons have no charge.

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6 0
3 years ago
Butane (C4 H10(g), mc031-1.jpgHf = –125.6 kJ/mol) reacts with oxygen to produce carbon dioxide (CO2 , mc031-2.jpgHf = –393.5 kJ/
ankoles [38]

The balanced chemical equation for the combustion of butane is:

2C_{4}H_{10}(g) +13 O_{2}(g)-->8CO_{2}(g)+10H_{2}O(g)

ΔH_{reaction}^{0} = Σn_{products}ΔH_{f}^{0}_{(products)}-Σn_{reactants}ΔH_{f}^{0}_{(reactants)}

                         = [{8*(-393.5kJ/mol)}+{10*(-241.82kJ/mol)}]-[{2*(-125.6kJ/mol)}+13*(0 kJ/mol)}]=[-3148kJ/mol+(-2418.2kJ/mol)]-[(-251.2kJ/mol)+0]

                      = -5315 kJ/mol

Calculating the enthalpy of combustion per mole of butane:

1mol C_{4}H_{10}*( \frac{-5315kJ}{2mol C_{4}H_{10} })=-2657.5 \frac{kJ}{molC_{4}H_{10}}

Therefore the heat of combustion per one mole butane is -2657.5 kJ/mol

Correct answer: -2657.5 kJ/mol

6 0
3 years ago
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