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Although we don't know the exact pH because we don't have any concentrations we know that NaHCO3 is a weak acid, and NaOH is a strong base.
Thus we should get a solution that becomes more basic so the pH > 7.
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∙ 9y ago
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Why there is a steep rise in the pH of acetic acid on titrating it with NaOH?
that is due to acetic acid is a weak acid and sodium hydroxide is a strong base. hence when they are titrated pH increases
What is the chemical equation for the neutralization reaction of HCl titrated with NaOH?
HCl + NaOH -----> NaCl + H2O
What is the molarity of an naoh solution if 4.37ml is titrated by 11.1 ml of 0.0904 m hno3?
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
What is the pH of NaHCO3?
NaHCO3 (Sodium bicarbonate) [at room temperature] will produce a pH of around 8.
Best indicator for lactic acid when titrated against standard NaOH?
phenolphthalein.
Why there is a steep rise in the pH of acetic acid on titrating it with NaOH?
that is due to acetic acid is a weak acid and sodium hydroxide is a strong base. hence when they are titrated pH increases
What is the chemical equation for the neutralization reaction of HCl titrated with NaOH?
HCl + NaOH -----> NaCl + H2O
What is the molarity of an naoh solution if 4.37ml is titrated by 11.1 ml of 0.0904 m hno3?
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
What is the pH of NaHCO3?
NaHCO3 (Sodium bicarbonate) [at room temperature] will produce a pH of around 8.
Best indicator for lactic acid when titrated against standard NaOH?
phenolphthalein.
A buffer is prepared by mixing 50.0 ml of 0.050 m sodium bicarbonate and 10.7 ml of 0.10 m naoh what is the pH for carbonic acid ka1 equals 4.5 x 10 -7 and ka2 equals 4.7 x 10 -11?
0.050M x .05L = .0025 mol NaHCO3 0.10M x .0107L = .00107 mol NaOH Excess NaHCO3 = .0025-.00107 = 0.00143 pH = pKa2 + log(.00107/.00143) pH = 10.20
A 0.361 molar solution of the weak acid HA with a pKa of 4.039 is titrated with a 0.163 molar solution of NaOH. What is the pH of the solution at the equivalence point of this titration?
You need to know the volume of the weak acid being titrated so you can find how many moles of base are needed to match that of the acid.
A 50.0 ml sample of 0.43 m benzoic acid c6h5cooh is titrated with 0.50 m naoh calculate the pH at the equivalence point ka of c6h5cooh equals 6.5 10-5?
8.78
What is the products when amidosulphuric acid is titrated with sodium hydroxide?
H3NO3S + NaOH → Na3NO3S + H2O
How much NaOH do you use to lower pH?
You dont - adding NaOH increases pH.
What is the pH of a 1 millimolar NaOH soluiton?
1 millimolar = 0.001 M NaOH ( a base, remember ) - log(0.001 M NaOH) = 3 14 - 3 = 11 pH ----------
What is the pH for sodium bicarbonate?
Sodium bicarbonate, NaHCO3 is alkaline so the pH will be greater than 7. However, the actual pH will depend on the concentration of the NaHCO3 solution.
