0
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.
Wiki User
∙ 13y ago
Wiki User
∙ 9y agoThe pH of 15 mL of 0.0045 M HNO3 is 2.35. The pOH is 11.7. When a solution has a pH under 7, it is said to be acidic.
Wiki User
∙ 10y agoTake the minus log value.So pH is equal to 1.
Wiki User
∙ 11y agoabout 11.2 pH
Wiki User
∙ 13y agopH = 1
Wiki User
∙ 11y ago1.64
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What is the pH of 2M HNO3?
pH= -log [H+] = -log [1] = 0
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 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.
What is the pH of 2M HNO3?
pH= -log [H+] = -log [1] = 0
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 )
Calculate the pH of 100 ml of a buffer that is 0.060 m NH4Cl and 0.115 m NH3 before and after the addition of 1 ml of 5.30 m HNO3?
pH = pKa - log([HA]/[A])[HA] = concentration weak acid NH4+ and [A] = concentration of weak base NH3 Before HNO3 addition [HA]= 6.0 mmol NH4+ in 100 ml => after: [HA]= 6.0+5.3 mmol NH4+ in 101 mlBefore HNO3 addition [A]= 11.5 mmol NH3 in 100 ml => after: [HA]= 11.5-5.3 mmol NH3 in 101 mlThus: (notice that pH of buffer is independent from a large range of dilution)pHbefore = 9.24- log10(6.0/100 / 11.5/100) = 9.24 - log10(6/11.5) = 9.52and:pHafter = 9.24 - log10(11.3/101 / 6.2/101) = 9.24 - log10(11.3/6.2) = 8.98
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 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 will be the final pH if you mix 500 ml of water with the water of 500 ml having pH 7?
7
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).
Is pH a extensive or intensive property?
pH is an INTENSIVE property as it does not depend on the amount of material present. The pH of 1 ml of solution x is the same as the pH of 100 ml of solution x.
How fast can a great white shark swim per hour?
It actually depends on what type of shark it is, and its speed it.
