In 0.01 M of HCl, the concentration of the Hydronium ions is 0.01M as well since HCl is monoprotic.
pH = -log [H3O+]
= -log 0.01
= -log10-2
= -(-2log10) = 2
Thus, the pH of 0.01 M HCl is 2.
pH = -log10[H+]
pH = -log10[2]
pH =2
You mean 0.1 M HCl?
-log(0.1 M HCl)
= 1 pH
In theory ZERO 0 -in practice about 0.1
its PH is 3
2
1,2
1N - conc will change the pH too quickly. You might want to consider 0.1molar for finer adjustments.
pH = -log10[H+], where [H+] is the hydrogen ion concentration. So, in this case, pH = -log10[1], yielding pH = 0.
Its pH value is 2.
It doesn't matter how much you have, HCl (Hydrochloric Acid) has a pH of 1
Hydrochloric Acid (HCl) pH of 1
1N - conc will change the pH too quickly. You might want to consider 0.1molar for finer adjustments.
pH = -log10[H+], where [H+] is the hydrogen ion concentration. So, in this case, pH = -log10[1], yielding pH = 0.
Its pH value is 2.
Yes, 0.1 M HCl has pH value of 1.0, 1.0 M HCl has pH value of 0.0, 10.0 M pH = -1.0 (even negative is possible, but this is about the limit)
It doesn't matter how much you have, HCl (Hydrochloric Acid) has a pH of 1
Hydrochloric Acid (HCl) pH of 1
Take specific volume of 3N solution and increase the volume three times by adding distilled water.
THE PH VALUE ACIDIC SOLUTION VARIOUS FROM 0-6.9, WHILE THE BASIC SOLUTION VARIOUS FROM 7.1-1.4. THUS ,OUT OF HCL AND NaOH WILL HIGHER PH VALUE
1N HCl is also 1M HCl because it is mono-protic. Therefore 36.5 g of HCl is required per liter or 3.65%. Simply take 100 g of 37% HCl and make up to the 1 liter mark on the volumetric flask. Check the value by titration against 1M NaOH. It should be perfect. If very slightly strong dilute very slightly (calculate) with water and re-standardize.
- log(0.25 M HCl) = 0.6 pH ------------
- log(0.00450 M HCl)= 2.3 pH=======
14Type your answer here...