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Can oxalic acid be titrated by HCl?
Yes, oxalic acid can be titrated by HCl because oxalic acid is a diprotic acid and can react with HCl in a simple acid-base reaction. The titration involves determining the volume of acid required to neutralize the oxalic acid solution, which can be used to calculate the concentration of oxalic acid.
How much acid is required to neutralise pH level11.2?
As many as hydroxide concentration:[OH-] = 10-[14.0-pH] = 10-[14.0-11.2] = 10-2.8 =invlog(-2.8) = 1.6*10-3 mol/LSo, to neutralize you've to add 1.6*10-3 mole strong monoprotic acid (H+) to 1.0 L solution of pH 11.2
What mass of potassium hydroxide is required to neutralize 95.00ml of 0.025m nitric acid?
The answer is o,13 g KOH.
Why addition of sodium carbonate required in method esterification?
Strong base is added to neutralize the strong acid (H2SO4).
Indicator used in TBN?
The primary indicator used in Total Base Number (TBN) testing is the amount of acid (often sulfuric acid) required to neutralize the basic components present in a lubricant sample. This indicates the alkalinity reserve of the lubricant, which can help determine its ability to neutralize acids formed during combustion in an engine.
What volume of the acid is required to neutralize the base?
Well,i guess the same volume as the base.
What volume of a 0.152 M potassium hydroxide solution is required to neutralize 10.2 ml of a 0.198 M hydrochloric acid solution?
To determine the volume of potassium hydroxide solution needed to neutralize the hydrochloric acid solution, you can use the formula M1V1 = M2V2. By plugging in the given values, you can calculate the volume of the potassium hydroxide solution required. In this case, the volume of the 0.152 M potassium hydroxide solution needed to neutralize 10.2 ml of the 0.198 M hydrochloric acid solution would be 7.43 ml.
What volume of 0.0550 M calcium hydroxide is required to neutralize 35.00 mL of 0.0550 M nitric acid?
To determine the volume of calcium hydroxide needed to neutralize the nitric acid, you can use the equation n1v1=n2v2, where n is the number of moles and v is the volume. As the concentration and volume are given for both the acid and base, the volumes of both solutions needed to neutralize each other will be equal. Therefore, the volume of 0.0550 M calcium hydroxide required will also be 35.00 mL.
What is hypothesis of a acid base titration?
The hypothesis of an acid-base titration is that the volume of the acid solution needed to neutralize a base solution is stoichiometrically equivalent to the volume of the base solution required to neutralize the acid. This forms the basis for determining the unknown concentration of an acid or base by titration.
What volume of NaOH solution (in mL) is needed to neutralize a given acid solution?
To determine the volume of NaOH solution needed to neutralize an acid solution, you would need to know the concentration of the acid solution and the volume of the acid solution. Using the equation n1V1 n2V2, where n represents the number of moles and V represents the volume, you can calculate the volume of NaOH solution needed.
How many ml of 250 M NaOH are required to neutralize 30.4 ml of 152 M HCl?
To neutralize the acid, we need to use the same number of moles of base. First, calculate the number of moles of HCl using its concentration and volume. Then, use the mole ratio from the balanced equation to find the required volume of NaOH. Convert the volume to mL.
What volume of base is needed to neutralize a strong acid?
Use this to analyse the unkown and variables:Ca*Va = Cb*Vb in which:C = concentration (mol/L = mmol/mL)V = Volume (L or mL)subscripts: 'a' = acid, 'b' = baseWanna know Vb ? well find the other three variables to calculate: (Ca*Va)/Cb = Vb (with the same unit as used for Va)
Can oxalic acid be titrated by HCl?
Yes, oxalic acid can be titrated by HCl because oxalic acid is a diprotic acid and can react with HCl in a simple acid-base reaction. The titration involves determining the volume of acid required to neutralize the oxalic acid solution, which can be used to calculate the concentration of oxalic acid.
How much acid is required to neutralise pH level11.2?
As many as hydroxide concentration:[OH-] = 10-[14.0-pH] = 10-[14.0-11.2] = 10-2.8 =invlog(-2.8) = 1.6*10-3 mol/LSo, to neutralize you've to add 1.6*10-3 mole strong monoprotic acid (H+) to 1.0 L solution of pH 11.2
What is the set up for an acid base titration?
In an acid-base titration, a known volume of acid or base of unknown concentration is titrated with a standardized solution of base or acid of known concentration, respectively. The setup involves adding an indicator to the solution being titrated, which changes color at the endpoint when the reaction is complete. The volume of the standardized solution required to neutralize the unknown solution is used to calculate its concentration.
What would require the largest volume of 0.100M sodium hydroxide solution for neutralization?
The largest volume of 0.100M sodium hydroxide solution would be needed to neutralize a strong acid with a low molarity. This is because a lower molarity acid would require more moles of sodium hydroxide to neutralize it, resulting in a higher volume of the solution being needed.
What mass of potassium hydroxide is required to neutralize 95.00ml of 0.025m nitric acid?
The answer is o,13 g KOH.
