Based on <span> Henderson - Hasselbach equation, we have
pH = pka + log </span>
Given: pH = 5.28 and [Acid] = 0.05 m,
∴ pKa = 5.28 - log (0.05) = 6.58
∴ Ka = 2.624 X
Thus, ionization constant of boric acid is 2.624 X
When the dissociation equation of NH3 is:
NH3(aq) + H2O ↔ NH4(aq) + OH-(aq)
when Kb =(1.8 x 10^-5)
and when PH+POH= 14
∴ POH = 14 -11= 3
when POH = -㏒[OH]
∴[OH] = 0.001
when [OH] = [NH4+] = 0.001
when Kb = [NH4+][OH-]/[NH4OH]
by substitution:
1.8 x 10^-5 = (0.001)^2 / [ NH4OH]
∴[NH4OH] = 0.06 M
Answer:
Mass ratio of magnesium = 2 : 1
Explanation:
Let us write down the masses of element involve to form the compounds .
Compound A → 7.88 g of mg and 15.68 g of 02
Compound B → 2.12 g of mg and 6.91 g of 02
since we want to get the mass ratio of magnesium, we divide the mass of mg with the other element present (oxygen) . we want to make both compound in equal proportions.
Compound A → 7.88 / 15.68 = 0.5025510204 g of Mg
/1 g of Oxygen
Compound B → 2.12 / 6.91 = 0.30680173661 g of Mg/ 1 g of Oxygen
Mass ratio of magnesium = compound A(Mg)/compound B(Mg)
Mass ratio of magnesium = 0.5025510204/0.30680173661
Mass ratio of magnesium = 1.63803186368
/1
Mass ratio of magnesium = 2 : 1
Answer:
Assign oxidation numbers to all atoms in the equation.
Compare oxidation numbers from the reactant side to the product side of the equation.
The element oxidized is the one whose oxidation number increased.
Explanation: