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Mumz [18]
3 years ago
11

2.643 grams of potassium butanoate (KCH3(CH2)2CO2 ) is fully dissolved in 50.00 mL of water, which is carefully transferred to a

conical flask. Then 100.00 mL of 0.120 M HCℓ is added dropwise to this solution from a burette. Given: Ka(butanoic acid) = 1.5 × 1O−5 . 2.1 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above.
Chemistry
1 answer:
lara [203]3 years ago
7 0

Answer:

The pH of the solution is 4.69

Explanation:

Given that,

Mass of potassium = 2.643 grams

Weight of water = 50.00 mL

Weight of HCl=100.00 ml

Mole = 0.120 M

We know that,

KCH_{3}(CH_{2})_{2}CO_{2} is a basic salt.

Let's write it as KY.

The acid HCH_{3}(CH_{2}CO_{2}) would become HY.

We need to calculate the moles of KY

Using formula of moles

moles\ of\ KY=\dfrac{m}{M}\times1000

moles\ of\ KY=\dfrac{2.643}{126}\times1000

moles\ of\ KY=20.97\ m\ mole

The reaction is

KY+HCl\Rightarrow HY+ KCl

The number of moles of KY is 20.98 m

initial moles = 20.98

Final moles m=20.98-0.120\times100= 8.98

We need to calculate the value of pKa(HY)

Using formula for pKa(HY)

pKa_{HY}=-log Ka

pKa_{HY}=-log(1.5\times10^{-5})

pKa_{HY}=4.82

We need to calculate the pH of the solution

Using formula of pH

pH=pKa+log(\dfrac{[KY]}{[KH]})

Put the value into the formula

pH=4.82+log(\dfrac{8.98}{12})

pH=4,69

Hence, The pH of the solution is 4.69

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Marysya12 [62]

Answer:

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Substance at the end of a reaction- product

Number placed before a compound in a chemical equation- stoichiometric coefficient

Explanation:

In a reaction equation, the species written on the left hand side of the equation are called the reactants.

The reactants combine to form the species on the right hand side of the reaction equation called products.

The stoichiometric coefficient is a number written before the formula of a compound in the reaction equation.

5 0
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For the generic equilibrium HA(aq) ⇌ H+(aq) + A−(aq), which of these statements is true? For the generic equilibrium , which of
timama [110]

<u>Answer:</u> The correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.

<u>Explanation:</u>

Common ion effect is defined as the effect which occurs on equilibrium when a common ion (an ion which is already present in the solution) is added to a solution. This effect generally decreases the solubility of a solute.

Equilibrium reaction of HA and KA follows the equation:

HA\rightleftharpoons H^{+}(aq.)+A^{-}(aq.)

KA\rightleftharpoons K^+(aq.)+A^{-}(aq.)

According to Le-Chateliers principle, if there is any change in the variables of the reaction, the equilibrium will shift in the direction in order to minimize the effect.

In the equilibrium reactions, A^- ion is getting increased on the product side, so the equilibrium will shift in the direction to minimize this effect, which is in the direction of HA.

Thus, the addition of KA will shift the equilibrium in the left direction.

Equilibrium constant depends on the temperature of the system. It does not have any effect on any change of pH.

pH is defined as the negative logarithm of hydrogen ions present in the solution

  • If the solution has high hydrogen ion concentration, then the pH will be low.
  • If the solution has low hydrogen ion concentration, then the pH will be high.

As, the equilibrium is shifting in the left direction, that means concentration of H^+ ions are getting decreases. This will increase the pH of the solution.

Hence, the correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.

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Explanation:

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Alekssandra [29.7K]

Answer:

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Explanation:

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The most stable monatomic Mg ion is Mg²⁺.

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ivanzaharov [21]
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