0
pH= -log [H+]
= -log [1]
= 0
Wiki User
∙ 12y ago
Wiki User
∙ 13y agoHNO3 is a strong mono-protic acid.
This means it fully ionises to NO3- and H+
Therefore the concentration of H+ = 1.0M
pH = -log[H+] = -log(1.0) = 0
pH = 0
Wiki User
∙ 10y ago12
(I reactly did a lab procedure and I tested it)
Wiki User
∙ 12y agoHNO3 → H+ + NO3-
2M HNO3 = 2M H+
pH = -log[H+] = -log[2] = -0.301
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What is the pH of 15 mL of 0.0045 M HNO3?
pH = - log10 [H+], where [H+] is the molar concentration of hydrogen ions. HNO3 is a strong acid and dissociates completely in water so a 5 M solution of HNO3 would have a concentration of hydrogen ions of 5M also. So, pH = -log10[5] = -0.699 which indicates an extremely strong acid.
What is the pH of 2M hcl?
- log (2) = - 0.3
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
What is the pH of a 0.01 M solution of the acid HNO3 in water?
- log(0.01 M HNO3) = 2 pH =====
What is the pH of a 1.6 10-3 M HNO3 solution?
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
What is the pH of 15 mL of 0.0045 M HNO3?
pH = - log10 [H+], where [H+] is the molar concentration of hydrogen ions. HNO3 is a strong acid and dissociates completely in water so a 5 M solution of HNO3 would have a concentration of hydrogen ions of 5M also. So, pH = -log10[5] = -0.699 which indicates an extremely strong acid.
What is the pH of 2M hcl?
- log (2) = - 0.3
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
What is the pH of a 0.01 M solution of the acid HNO3 in water?
- log(0.01 M HNO3) = 2 pH =====
What is the pH of a 1.6 10-3 M HNO3 solution?
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
Why HNO3 is called a strong acid since its pH is less than that of H3O?
the lower the pH the stronger the acid
What is the molarity of a strong acid solution with a pH of 2?
1x10-2M
What is the fix pH of HCL and HNO3?
The pH value of those solutions depends on the concentration and the temperature. Generally, solutions with higher concentrations of acids have lower pH values.
How much 2.5 molarity of HNO3 is required to react the CaCO3?
This depends on the mass of calcium carbonate.
What is the pH of HNO3?
HNO3 is nitric acid. De[emdimng on its level of concentration it can vary from '0' (very concentrated ; 16M) to '3'. ) low concentration (dilute ' say 0.6 M).
What is hydrogen ion concentration of 0.5 HNO3?
0.5 mol H+ per Litre, pH = 0.3
What substances have the highest pH?
Concentrated bases (more than 2M/L) as sodium hydroxide for example.
