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pH = -log[H+]
That is, the pH of a solution is the negative log of the concentration of hydrogen atoms. The concentration of hydrogen atoms must be in units of Molarity, or moles per liter. In order to determine the pH of a solution containing 1 mole of HCl, you must also know the volume of the solution.
I am assuming the question is: What is the pH of 1M HCl, and not 1 mole. 1 mole HCl is simply the mass in grams of the atomic weight of H and Cl: 1+35.45=36.45. This is not a unit of concentration and if that is truly the question then the answer is undefined.
Molarity on the other hand, and other units of concentration, are completely independent of total amount of solution (volume or mass): molarity (M)= moles/Liters
HCl is a strong acid. This means that all of those acid hydrogens are releasing into solution and therefore the calculation is very simple:
pH of strong acid= -log[H+] 1M HCl= 1M[H+] + 1M[Cl-] pH=-log[1]= 0
Wiki User
∙ 9y ago
Wiki User
∙ 12y agopH= -log [H+]
= -log [1]
= 0
Wiki User
∙ 12y agoThe pH of a .1M solution of HCI is 1. HCI is a strong elctrolyte, -log(.1)=1
Answer from PCH.com
Wiki User
∙ 9y ago4.01 is the amount of pH in a 1.5 M HCl solution.
Wiki User
∙ 11y ago- log(1 X 10 -4 M HCl)
= 4 pH
=====
Wiki User
∙ 10y agoYou use this formula. PH = - log [H+]. And this is a strong acid so it dissolve absolutely into H+.
P/s: the answer is 6
Wiki User
∙ 13y agopH = 0.0 (zero)
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What is the pH of a 0.1 mole per liter HCl solution?
1 (one).
What If enough water is added to 5 g of HCl to make 1 liter of solution what is the pH?
Find moles HCl. 5 g HCl (1 mole HCl/36.450 grams) = 0.1372 moles HCl Now, Molarity = moles of solute/Liters of solution Molarity = 0.1372 moles HCl/1 liter = 0.1372 M HCl Then. -log(0.1372 M HCl) = 0.9 pH ( you might call it 1, but pH can be off the scale ) -----------
What is the pH of a solution that contains 0.10 mole of HCI in a voulme of 100.0l?
100 Liters? I will assume as much. Molarity = moles of solute/Liters of solution Molarity = 0.10 mole HCl/100.0 Liters = 0.001 M HCl -------------------------now, to find pH - log(0.001 M HCl) = 3 pH -----------------so, your acid is of 3 pH, which is to be expected at the volume od solution
What is the concetration of 400 ml of 0.5 M HCl?
Since the molecular weight of HCl is 36.46g/mole, 1 mole of HCl contains 36.46g. 1 liter of a 0.5M solution will have 18.23g of HCl. 400 ml will have 7.292g of HCl.
What is the limiting reactant of 0.5 mol of zinc to 0.75 mol of hydrochloric acid?
Balanced equation first.Zn + 2HCl --> ZnCl2 + H20.5 mole Zn (2 moles HCl/1 mole Zn)= 1 mole HCl================you do not have this much moles HCl0.75 moles HCl (1 mole Zn/2 mole HCl)= 0.375 moles Zn===================you have more moles Zn than thisSo. HCl limits this reaction.
What is the pH of a 0.1 mole per liter HCl solution?
1 (one).
What has the pH of 1?
pH=1 means the solution contains 0.1 mole per liter H+ ions. Strong acids like hydrochloric acid (HCl) or sulfuric acid (H2SO4) dissociate completely in water so 0.1 mole of HCl (= 3,65 g per liter) has a pH=1. For sulfuric acid 0.1 mole = 9.8 g per liter give pH =1
Show my the pH chart by strong and weak acid?
A strong acid completely dissociates into an H+ ion and an anion. pH is defined as pH = -log(H+ concentration) So if you have 0.01 mole hydrochloric acid (HCl) per 1 mole solution, since each mole HCl contributes a mole of H+ and a mole of Cl- then you would have H+ concentration of 0.01 pH = -log(0.01) = -(-2) = 2, so the pH = 2 Note that higher H+ concentrations result in lower pH number
What If enough water is added to 5 g of HCl to make 1 liter of solution what is the pH?
Find moles HCl. 5 g HCl (1 mole HCl/36.450 grams) = 0.1372 moles HCl Now, Molarity = moles of solute/Liters of solution Molarity = 0.1372 moles HCl/1 liter = 0.1372 M HCl Then. -log(0.1372 M HCl) = 0.9 pH ( you might call it 1, but pH can be off the scale ) -----------
What is the pH of a solution that contains 0.10 mole of HCI in a voulme of 100.0l?
100 Liters? I will assume as much. Molarity = moles of solute/Liters of solution Molarity = 0.10 mole HCl/100.0 Liters = 0.001 M HCl -------------------------now, to find pH - log(0.001 M HCl) = 3 pH -----------------so, your acid is of 3 pH, which is to be expected at the volume od solution
What is the concetration of 400 ml of 0.5 M HCl?
Since the molecular weight of HCl is 36.46g/mole, 1 mole of HCl contains 36.46g. 1 liter of a 0.5M solution will have 18.23g of HCl. 400 ml will have 7.292g of HCl.
What is the limiting reactant of 0.5 mol of zinc to 0.75 mol of hydrochloric acid?
Balanced equation first.Zn + 2HCl --> ZnCl2 + H20.5 mole Zn (2 moles HCl/1 mole Zn)= 1 mole HCl================you do not have this much moles HCl0.75 moles HCl (1 mole Zn/2 mole HCl)= 0.375 moles Zn===================you have more moles Zn than thisSo. HCl limits this reaction.
What is theoretical pH value for 1 m hcl solution?
It doesn't matter how much you have, HCl (Hydrochloric Acid) has a pH of 1
What is the pH of 260M HCl?
.260 M of HCL, not 260 More than likely correct, but, - log(0.260 M HCl) = 0.6 pH ----------- ( pH can be below 1 )
How many moles HCl in 8.3 g HCl?
8.3 grams HCl (1 mole HCl/36.458 grams) = 0.23 moles HCl ------------------------
How many moles of CuO are needed to react with 4 moles of HCL?
4 mole cuO X 2/1 = 8 mole Hcl
How many moles of hcl are needed to react with 4 moles of cuo?
4 mole cuO X 2/1 = 8 mole Hcl
