The pH of a 0.6 M HNO3 solution is approximately 0.23. This is because nitric acid is a strong acid that completely ionizes in solution, resulting in a high concentration of H+ ions that lower the pH.
- log(0.01 M HNO3) = 2 pH =====
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
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.
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.
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 )
- log(0.01 M HNO3) = 2 pH =====
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
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.
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.
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 )
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.
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.
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The reaction between HNO3 and NaOH is a 1:1 molar ratio. This means that the moles of HNO3 required to neutralize the NaOH is the same as the moles of NaOH. Given that 20.0 ml of HNO3 is needed to neutralize 10.0 ml of a 1.67 M NaOH solution, the molarity of the HNO3 solution is twice the molarity of the NaOH solution, which is 3.34 M.
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
HNO3 is a strong acid, which means it dissociates completely. This means you don't have to set up an equilibrium scenario; you can just go with the given molarity as also being the concentration of hydrogen ions [H+]. So, pH = -log(0.00884), which is about 2.05.
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!).