<span>To determine the pH of the solution given, we make
use of the acid equilibrium constant (Ka) given. It is the ratio of the
equilibrium concentrations of the dissociated ions and the acid. The
dissociation reaction of the CH3COOH acid would be as follows:
</span>CH3COOH = CH3COO- + H+<span>
The acid equilibrum constant would be expressed as follows:
Ka = [H+][</span>CH3COO-] / [CH3COOH] = 1.8× 10^–5
<span>
To determine the equilibrium concentrations we use the ICE table,
CH3COOH H+ </span>CH3COO<span>-
I 1.60 0 0
C -x +x +x
----------------------------------------------------------------
E 1.60-x x x
</span>1.8× 10^–5 = [H+][CH3COO-] / [CH3COOH] <span>
1.8 x 10^-5 = [x][x] / [0.160-x] </span>
Solving for x,
x = 1.69x10^-3 = [H+] = [F-]
pH = -log [H+] = -log [1.69x10^-3] = 2.8
Answer:
3H2SO4 + 2B(OH)3 -> B2(SO4)3 + 6H2O
Explanation:
Ionic bounds are formed due to the electrostatic attraction between oppositely charged ions in a chemical compound.
The atom that loses the electrons becomes a positively charged ion (cation), while the one that gains them becomes a negatively charged ion (anion).
molecule (hope this helps :))
