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Why there is a steep rise in the pH of acetic acid on titrating it with NaOH?
The steep rise in pH of acetic acid when titrated with NaOH occurs near the equivalence point because at that point nearly all the acetic acid has been neutralized, resulting in a rapid increase in pH from the addition of hydroxide ions. This phenomenon is due to the buffering capacity of acetic acid being overwhelmed as it reacts with the base to form acetate ions.
Is salicylic acid miscible in Naoh nahco3 and Hcl?
Salicylic acid is soluble in NaOH and insoluble in NaHCO3 and HCl. In NaOH, salicylic acid can form a salt through neutralization. In NaHCO3 and HCl, salicylic acid remains as a solid due to its low solubility in these solutions.
Why use NaHCO3 for iodometric titration?
Sodium bicarbonate (NaHCO3) is used in iodometric titration as a reaction enhancer to neutralize excess acids that may interfere with the redox reaction between iodine and the analyte being titrated. By maintaining a slightly basic pH, NaHCO3 helps stabilize the iodine solution, ensuring more accurate and reliable results.
Best indicator for lactic acid when titrated against standard NaOH?
The best indicator for titrating lactic acid against standard NaOH is phenolphthalein. It changes color in the pH range of about 8.2 to 10, which is suitable for the endpoint of the titration of lactic acid (pKa ≈ 3.9). This indicator appears pink at high pH and colorless at acidic pH, allowing for a clear visual indication of the endpoint of the titration.
What is the pH of NaHCO3?
NaHCO3 (Sodium bicarbonate) [at room temperature] will produce a pH of around 8.
Why there is a steep rise in the pH of acetic acid on titrating it with NaOH?
The steep rise in pH of acetic acid when titrated with NaOH occurs near the equivalence point because at that point nearly all the acetic acid has been neutralized, resulting in a rapid increase in pH from the addition of hydroxide ions. This phenomenon is due to the buffering capacity of acetic acid being overwhelmed as it reacts with the base to form acetate ions.
Is salicylic acid miscible in Naoh nahco3 and Hcl?
Salicylic acid is soluble in NaOH and insoluble in NaHCO3 and HCl. In NaOH, salicylic acid can form a salt through neutralization. In NaHCO3 and HCl, salicylic acid remains as a solid due to its low solubility in these solutions.
Why use NaHCO3 for iodometric titration?
Sodium bicarbonate (NaHCO3) is used in iodometric titration as a reaction enhancer to neutralize excess acids that may interfere with the redox reaction between iodine and the analyte being titrated. By maintaining a slightly basic pH, NaHCO3 helps stabilize the iodine solution, ensuring more accurate and reliable results.
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
What is the products when amidosulphuric acid is titrated with sodium hydroxide?
H3NO3S + NaOH → Na3NO3S + H2O
Best indicator for lactic acid when titrated against standard NaOH?
The best indicator for titrating lactic acid against standard NaOH is phenolphthalein. It changes color in the pH range of about 8.2 to 10, which is suitable for the endpoint of the titration of lactic acid (pKa ≈ 3.9). This indicator appears pink at high pH and colorless at acidic pH, allowing for a clear visual indication of the endpoint of the titration.
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?
The pH of a 1 millimolar NaOH solution is approximately 11. The concentration of a 1 millimolar solution is 0.001 mol/L, and NaOH is a strong base that completely dissociates in water to produce hydroxide ions, leading to a basic pH.
What is the pH of NaHCO3?
NaHCO3 (Sodium bicarbonate) [at room temperature] will produce a pH of around 8.
How do you prepare Britton Robinson buffer?
Britton-Robinson buffer is a "universal" pH buffer used for the range pH 2 to pH 12. Universal buffers consist of mixtures of acids of diminishing strength (increasing pKa) so that the change in pH is approximately proportional to the amount of alkali added. It consists of a mixture of 0.04 M H3BO3, 0.04 M H3PO4 and 0.04 M CH3COOH that has been titrated to the desired pH with 0.2 M NaOH. Britten and Robinson also proposed a second formulation that gave an essentially linear pH response to added alkali from pH 2.5 to pH 9.2 (and buffers to pH 12). This mixture consists of 0.0286 M citric acid, 0.0286 M KH2PO4, 0.0286 M H3BO3, 0.0286 M veronal and 0.0286 M HCl titrated with 0.2 M NaOH.
What is the PH of 0.001N NaOH?
The pH of a 0.001N NaOH solution is around 11.9. NaOH is a strong base, and at this concentration, it will result in a highly alkaline solution.
What is the pH of Pepsin in NaOH?
The pH of pepsin in NaOH would depend on the concentration of NaOH added. Pepsin is an enzyme that functions best at acidic pH levels, around pH 2.0. Adding NaOH, a base, would increase the pH, potentially inactivating the pepsin enzyme as it moves away from its optimal pH range for activity.
