Question

Calculate pH: 5.00 mL of 1.20 M  HCl diluted to 0.440 L & A mixture formed by adding 42.0 mL of 1.5×10⁻²M  HCl to 160 mL of 1.0×10⁻²M  HI.

The equilibrium constant Kc for C(s)+CO2(g)⇌2CO(g) is 1.9 at 1000 Kand 0.133 at 298 K. How many grams of C are consumed?

Answer 1

1.

0.00500 Litres of 1.2 mol / litre HCl = 0.00600 moles of HCl
diluted to 0.440 L:
0.00600 moles of HCl / 0.440 Liters = 0.0136 Molar HCl

pH = - log of 0.0136 Molar H+
pH = 1.87

2.
pH of a mixture formed by adding
0.160 L of 0.015 M HCl = 0.0024 moles of HCl
0.0024 moles of HCl releases 0.0024 moles of H+

0.160 L of 0.010 mol/Litre HI = 0.0016 moles of HI
0.0016 moles of HI releases 0.0016 moles of H+

0.0024 moles of H+ & 0.0016 moles of H+ = 0.004 moles of H+
find molarity of the total 202 ml volume:
0.004 moles of H+ / 0.202 Litres = 0.01980 Molar H+

pH = - log of 0.01980 Molar H+
pH = 1.70

Second problem is incomplete. Grams of CO2 should be given.