Normality= molarityX total POSITIVE oxidation number of solute Solvent=substance present in the greatest amount Solute= all other substances in the solution +1 (1 na+) is the total POSITIVE oxidation number of NaOH 2.0X1= 2.0 N=2.0
pH = -log [H+ ion concentration]
HNO3 is a strong acid, and because it is strong you can just plug 2.0M in for the H+ ion concentration and solve.
If it were a strong base, you would take the answer you got for the above problem as your pOH instead of pH. pOH+pH=14. This method only works for strong acids or bases.
Since each NaOH molecule contains only one hydroxide ion, the normality of NaOH is equal to its molarity. Therefore, 1.0 N of NaOH is the same as 1 M.
NaOH 1.0 N (normal) is standardised at 1.0 mole per Liter
12
In the following reaction calculate and find the normality of the solution when 1.0 M H3PO4 reacts with NaOH?
H3AsO4 + 2NaOH → Na2HAsO4 + 2H2O
- 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.
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 )
its 7, seven is neutral.
- 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.
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 )
its 7, seven is neutral.
10
1/103.4= 4.0 x 10 -4 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.
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
its PH is 3
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