In a beaker containing 100 ml of water, equal moles of HCl and Ca(OH)2 are mixed. The resulting solutions contains mainly which of the following?
A) water and CaCl2
B) water and Cl-, Ca +2, and H+ ions
C) water and H+, Cl-, Ca+2 and OH- ions
D) water, HCL and Ca(OH)2
E) water, Cl-, Ca+2 and OH- ions
2006-10-08 16:43:23 · 3 answers · asked by Anonymous in Education & Reference ➔ Homework Help
HCl is a STRONG ACID, it WILL ionize completely.
Ca(OH)2 is a STRONG BASE, it WILL ionize completely.
SO the answer is C
If you know your strong acids (8 of them) and the two strong base groups these are easy.....if they are weak, they will not completely ionize.
STRONG ACIDS:
HCl
HBr
HI
HIO4
HClO3
HClO4
H2SO4
HNO3
Strong Bases:
Group IA hydroxides--all of them
calcium , strontium, barium hydroxides...all heavy Group IIA metals
2006-10-08 16:48:57 · answer #1 · answered by Anonymous · 0⤊ 0⤋
The answer is A) water and CaCl2.
For a complete reaction, you need:
2HCI + Ca(OH)2 -> 2H2O + CaCl2
In this reaction, all of the HCI is consumed and one half of the Ca(OH)2 is consumed. You're left with water, salt and the remaining base, but the solution "mainly" contains water and CaCl2.
2006-10-09 00:14:10 · answer #2 · answered by mozart 3 · 1⤊ 0⤋
Mozart is correct here he one smart Cookie and very helpful
2006-10-11 00:03:30 · answer #3 · answered by Magnusfl 3 · 0⤊ 0⤋