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KIM [24]
3 years ago
6

A solution is prepared by mixing 0.12 moles of acetic acid with 0.22 moles of sodium acetate in 1.00 liters of solution. What wi

ll be the pH of the solution once equilibrium is established?
Chemistry
1 answer:
nataly862011 [7]3 years ago
6 0

Answer : The pH of the solution is, 5.01

Explanation :

For acetic acid : pK_a=4.75

First we have to calculate the concentration of acetic acid and sodium acetate.

Concentration of acetic acid (Acid) = \frac{Moles}{Volume}=\frac{0.12mol}{1.00L}=0.12M

Concentration of sodium acetate (salt) = \frac{Moles}{Volume}=\frac{0.22mol}{1.00L}=0.22M

Now we have to calculate the pH of the solution.

Using Henderson Hesselbach equation :

pH=pK_a+\log \frac{[Salt]}{[Acid]}

Now put all the given values in this expression, we get:

pH=4.75+\log (\frac{0.22}{0.12})

pH=5.01

Therefore, the pH of the solution is, 5.01

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What type of organic compound has the empirical formula CH2O and can serve as energy storage or the starting material for fats a
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Carbohydrates. CH2O is the most basic formula of simple sugars.Empirical formula is the lowest whole number ratio of atoms in a formula.For example glucose is C6H12O6 can be reduced by 6 to get CH2O. Simples sugars include glucose and fructose which can serve as sources of energy for fats and amino acids.
4 0
3 years ago
4Cr(s)+3O2(g)→2Cr2O3(s) calculate how many grams of the product form when 21.4 g of O2 completely reacts
weqwewe [10]

Answer:

= 67.79 g

Explanation:

The equation for the reaction is;

4Cr(s)+3O2(g)→2Cr2O3(s)

The mass of O2 is 21.4 g, therefore, we find the number of moles of O2;

moles O2 = 21.4 g / 32 g/mol

                =0.669 moles

Using mole ratio, we get the moles of Cr2O3;

moles Cr2O3 = 0.669 x 2/3

                       =0.446 moles

but molar mass of Cr2O3 is 151.99 g/mol

Hence,

The mass Cr2O3 = 0.446 mol x 151.99 g/mol

                            <u> = 67.79 g </u>

6 0
3 years ago
&amp; For the reaction A
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Answer:

The rate reduces by a factor cf /2.

5 0
3 years ago
You wish to prepare an HC2H3O2 buffer with a pH of 4.24. If the pKa of is 4.74, what ratio of C2H3O2 /HC2H3O2 must you use?
LenaWriter [7]

To solve this problem, we can use the Henderson-Hasselbalch Equation which relates the pH to the measure of acidity pKa. The equation is given as:<span>

<span>pH = pKa + log ([base]/[acid])                ---> 1</span></span>

Where,

[base] = concentration of C2H3O2 in molarity or moles

<span>[acid] = concentration of  HC2H3O2 in molarity or moles</span>

 

For the sake of easy calculation, let us assume that:

[base] = 1

[acid] = x

<span>
Therefore using equation 1,
4.24 = 4.74 + log (1 / x) 

<span>log (1 / x) = - 0.5

1 / x = 0.6065 </span></span>

x = 1.65<span>

The required ratio of C2H3O2 /HC2H3O2 <span>is 1:1.65 or 3:5. </span></span>
3 0
3 years ago
In Europe, nutritional information is given in kilojoules (kJ) instead of nutritional calories (1 nutritional calorie = 1 kcal).
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There would be 68 calories per cup
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