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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 concentration of HNO3 in a solution with pH3.4?
The concentration of HNO3 in a solution with pH 3.4 is approximately 3.98 x 10^-4 M. This is calculated using the formula pH = -log[H+], where [H+] is the hydrogen ion concentration in mol/L. For nitric acid (HNO3), one mole of HNO3 produces one mole of H+ in solution.
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 concentration of HNO3 in a solution with pH3.4?
The concentration of HNO3 in a solution with pH 3.4 is approximately 3.98 x 10^-4 M. This is calculated using the formula pH = -log[H+], where [H+] is the hydrogen ion concentration in mol/L. For nitric acid (HNO3), one mole of HNO3 produces one mole of H+ in solution.
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 hydrogen ion concentration of 0.5 HNO3?
A 0.5 M solution of HNO3 will have a hydrogen ion concentration of 0.5 moles per liter. This is because each molecule of HNO3 ionizes to produce one hydrogen ion in solution.
What is the pH of the solution formed by completely neutralizing 50 milliliters of 0.1 m hno3 with 50 milliliters of 0.1 m naoh at 298 k?
The reaction between HNO3 (acid) and NaOH (base) results in the formation of water and a salt, NaNO3. Since both the acid and base are of equal concentration and are completely neutralized, the resulting solution would be a neutral solution with a pH of 7.
How many moles of hno3 are needed to prepare 5.0 of a 2.0 m solution of hno3?
10
What would be pH of a 0.00884 M solution of HNO3?
To find the pH of a 0.00884 M solution of HNO₃ (nitric acid): HNO₃ is a strong acid, so it completely dissociates: HNO 3 ​ →H +NO 3 − ​ Therefore: [H ]=0.00884 M Use the pH formula: pH=−log[H ] pH=−log(0.00884) pH≈2.05 Answer: pH≈2.05 ​ The solution is acidic because nitric acid releases hydrogen ions in water.
What is the molarity of a solution dissolve 0.31 grams of HNO3 in 300ml of water?
Molarity = moles of solute/Liters of solution ( get moles of HNO3 and 300 ml = 0.300 Liters ) 0.31 grams Nitric acid (1 mole HNO3/63.018 grams) = 0.004919 moles HNO3 Molarity = 0.004919 moles HNO3/0.300 Liters = 0.0164 M HNO3
What is the pH of a 0.200 M solution of HNO3?
The definition of pH is the -log[H+], which basically means the negative common log (base 10) of the concentration of hydronium ions in solution. Since nitric acid is a strong monoprotic acid (one H+) it makes the problem so much easier since there is no acid equilibrium to deal with. Since there is one H+ for every acid molecule thus the [H+], or concentration of H+, is equal to the concentration of the acid, which is given to be 0.2004M. Thus, pH = -log[H+] = -log(0.2004) = (with sig figs) 0.6981 pH, something you really don't want to stick your hand in, but not as bad as some acid I've seen (yay, negative pH!).
What is the pH of a solution containing 0.1 M of HC2H3O2?
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
