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3 years ago

Examples of chemical changes in nature

2 answers:

7 0

rusting of ironcombustion (burning) of woodmetabolism of food in the bodymixing an acid and a base, such as hydrochloric acid (HCl) andsodium hydroxide (NaOH)cooking an eggdigesting sugar with the amylase in salivamixing baking soda and vinegar to produce carbon dioxide gasbaking a cakeelectroplating a metalusing a chemical batteryexplosion of fireworksrotting bananasgrilling a hamburgermilk going sour

Vadim26 [7]3 years ago

4 0

When a tree starts to rot

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Solid potassium hydroxide koh decomposes into gaseous water and solid potassium oxide . write a balanced chemical equation for t

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4 years ago

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3 years ago

Find the pH of a 0.100 molar H2C6O6 solution with ka, where KA is equal 8.0×10–5

lubasha [3.4K]

The pH of the solution is 2.54.

Explanation:

pH is the measure of acidity of the solution and Ka is the dissociation constant. Dissociation constant is the measure of concentration of hydrogen ion donated to the solution.

The solution of C₆H₂O₆ will get dissociated as C₆HO₆ and H+ ions. So the molar concentration of 0.1 M is present at the initial stage. Lets consider that the concentration of hydrogen ion released as x and the same amount of the base ion will also be released.

So the dissociation constant Kₐ can be written as the ratio of concentration of products to the concentration of reactants. As the concentration of reactants is given as 0.1 M and the concentration of products is considered as x for both hydrogen and base ion. Then the

$K_{a}=\frac{[H^{+}][HB] }{[reactant]}$

[HB] is the concentration of base.

$8 * 10^{-5} =\frac{x^{2} }{0.1}\\\\\\x^{2} = 8 * 10^{-5}*0.1$

$x^{2} = 0.08 * 10^{-4}\\ \\x = 0.283*10^{-2}$

Then

$pH = - log [x] = - log [ 0.283 * 10^{-2}]\\ \\pH = 2 + 0.548 = 2.54$

So the pH of the solution is 2.54.

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3 years ago