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A solution containing 3.76 g naoh in 361 ml water is titrated with 491 ml hcl what is the concentration of hcl in the original solution?
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∙ 9y ago
The concentration of hcl is 0.13.
Wiki User
∙ 9y ago
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50 ml of hcl is titrated with a solution of 0.24 m naoh it requires 35 ml of naoh to reach the equivalence point what is the concentration of the hcl solution?
.17
30 ml of hydrofluoric acid hf is titrated with a solution of 0.10 m koh if 55 ml of koh is required to reach the equivalence point what is the concentration of the acetic acid solution?
0.13 is the concentration of the acetic acid solution.
65 ml of hcl is titrated with a solution of 0.15 m koh it requires 44 ml of koh to reach the equivalence point what is the concentration m of the hcl solution?
0.1
20 ml of acetic acid ch3cooh is titrated with a solution of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
0.26
20 ml of acetic acid is titrated with a solution of 0.15 M NaOH If 35 ml of NaOH are required to reach the equivalence point what is the concentration of the acetic acid solution?
0.01 molar
What is the operation principle of a titration?
A solution containing an element to be determined (the concentration being unknown) is titrated (adding a reagent - the titrant) with a standard solution (with a known concentration); knowing the volume of the titrant and the reaction which occur the concentration of the analyte is calculated. Titration is manual (also called volumetry) or potentiometric and is a very common method in analytical chemistry.,
50 ml of hcl is titrated with a solution of 0.24 m naoh it requires 35 ml of naoh to reach the equivalence point what is the concentration of the hcl solution?
.17
30 ml of hydrofluoric acid hf is titrated with a solution of 0.10 m koh if 55 ml of koh is required to reach the equivalence point what is the concentration of the acetic acid solution?
0.13 is the concentration of the acetic acid solution.
65 ml of hcl is titrated with a solution of 0.15 m koh it requires 44 ml of koh to reach the equivalence point what is the concentration m of the hcl solution?
0.1
20 ml of acetic acid is titrated with a solution of 0.15 M NaOH If 35 ml of NaOH are required to reach the equivalence point what is the concentration of the acetic acid solution?
0.01 molar
20 ml of acetic acid ch3cooh is titrated with a solution of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
0.26
What is a secondary solution?
A solution that has been titrated against a primary standard solution.
A 25 ml sample of 723 m hclo4 is titrated with a 273 m koh solution the h3o concentration after 66.2 ml of koh is?
1.00x10^-7
What is the difference between aqueous and non aqueous titration?
Aqueous titration: the ion to be titrated is in an aqueous solution Nonaqueous titration: the ion to be titrated is in an nonaqueous solution
20ml of acetic acid is titrated with a solutuion of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
.26
How does the equivalence point differ from the half equivalence point?
Equivalence point is reached when Reactants react at Stoichiometric ratios and reach the Endpoint so that no more of the solution being titrated is found.Eg: Strong base + Strong Acid: HCL+NaOH--> NaCl+H2O1mol of Hcl Requires 1 mol of NaCl,Therefore 3.65 moles of Hcl Requires 3.65Moles of NaOH and equivalence point is reached when that much is added to the acid being titrated for example .Half Eq point is when Half of the Solution being titrated has reacted. It is a point on a titration curve which corresponds to the addition of exactly half of the volume of the titrant needed to reach equivalence point (or end point )Corrected:So, at HALF-WAY Eq. point the pH = pKa, since the actual concentration of ACID is equal to concentration of its conjugate BASE because both are equal to HALF of the original (unknown) acid concentration to be titrated (half left = half formed).
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.
