Answer:
kilograms
Explanation:
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Answer:
[2 ]Na+[2 ]H2O -> [ 2] NaOH + [1]H2
First, find moles of gold given the mass of the sample:
(35.9g Au)/(197.0g/mol Au) = 0.182mol Au
Second, multiply moles of Au by Avogrado's number:
(0.182mol)(6.02 x10^23)= 1.10x10^23 atoms Au
Answer:
31.78 grams
25.55%
Explanation:
The balanced reaction for ammonium chloride with calcium oxide will be:
2NH4Cl + Ca(OH)2 ---> CaCl2 + 2NH3 + 2H2O
The molecular weight for ammonium chloride(NH4Cl ) is 53.49g/mol, while the molecular weight for ammonium(NH3) is 17g/mol. The number of theoretical yield of ammonia from 100g of ammonium chloride will be:
100g / (53.49g/mol) * 2/2 * 17g/mol= 31.78 grams
If the actual yield is 8.12g, the percent yield will be: 8.12g/31.78g * 100% =25.55%
Answer:
pH = 3.02
Explanation:
Acetic Acid is a weak acid (HOAc) that ionizes only ~1.5% as follows:
HOAc ⇄ H⁺ + OAc⁻.
In pure water the hydronium ion concentration [H⁺] equals the acetate ion concentration [OAc⁻] and can be determined* using the formula [H⁺] = [OAc⁻] = SqrRt(Ka·[acid]) = SqrRt(1.8x10⁻⁵ x 0.0500)M = 9.5x10⁻⁴M.
By definition, pH = -log[H⁺] = -log(9.5x10⁻⁴) = 3.02
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*This formula can be used to determine the [H⁺] & [Anion⁻] concentrations for any weak acid in pure water given its Ka-value and the molar concentration of acid in solution.