Answer:
(i) Al2(SO4)3
(ii) CaCl2
(iii) Fe(OH)2
(iv)AlPO4
(v) Fe(NO3)3
(vi) AuCl3
(vii) AgNO3
Explanation:
The numbers after the element/ion is a subscript meaning its put below the symbol
(i) Al has a charge of 3+ and SO4 has a charge of 2-
So to balance the charges 2 Al is needed to make the charge a 6+ and 3 SO4 is needed to make the charge a 6-. Once you can add the two charge values together to create 0, then you have the correct quantities
(ii) Same applies here, but Ca is 2+ and Cl is 1-, so 2 Cl- is needed to balance out the Ca
(iii) Ferrous is an ion of Iron with a 2+ charge, the other ion of Iron is Ferric which has a 3+ charge. OH has a charge of -1, so 2 OH is needed to balance out one Fe
(iv) Aluminum again has a charge of 3+ while PO4 has a charge of 3-, so they both balance out with one of each.
(v) Ferric is an ion of iron with a charge of 3+ and NO3 has a charge of 1-, so three of NO3 is needed to balance.
(vi) Gold has two charges, 1+ or 3+. However used in Gold chloride it is a 3+ and Cl is a 1-, so 3 of Cl is needed to balance one gold.
(vii) Silver has a charge of 1+ while NO3 has a charge of 1-, so they balance each other at one each.
Answer:
Hydroxide concentration of the sample is 1.3x10⁻⁶M
Explanation:
The equilibrium constant of water, Kw, is:
H₂O(l) ⇄ H⁺(aq) + OH⁻(aq)
Kw is defined as:
Kw = 1.7x10⁻¹² = [H⁺] [OH⁻]
As the sample is of pure water, both H⁺ and OH⁻ ions have the same concentration because come from the same equilibrium, that is:
[H⁺] = [OH⁻]
We can write the Kw expression:
1.7x10⁻¹² = [OH⁻] [OH⁻]
1.7x10⁻¹² = [OH⁻]²
1.3x10⁻⁶M = [OH⁻]
<h3>Hydroxide concentration of the sample is 1.3x10⁻⁶M</h3>
