Chemistry-
General
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Question

the-dissociation of weak electrolyte (weak acid) is expressed in terms of Ostwald dilution law stronger is the acid, weaker is its conjugate base_ The dissociation constants of an acid (K subscript a end subscript) and its conjugate base (K subscript b end subscript ) are related by the given relation: -
K subscript w end subscript equals K subscript a end subscript cross times K subscript b end subscript
At 25 to the power of ring operator end exponent C comma K subscript w end subscript (Ionic product of water) equals 10 to the power of negative 14 end exponent
Phosphoric acid isa weak acid. It is used in fertilizer, food, detergent and toothpaste. Structure of phosphoric acid is:

Aqueous solution of phosphoric acid with a density oflg mL-1 containing 0.05% by weight of phosphoric acid is used to impart tart taste to many soft drinks. Phosphate ion is an inteife ring radical in qualitative analysis. It should be removed for analysis beyond third group of qualitative analysis
the basicity of phosphoric acid is:

  1. 1    
  2. 2    
  3. 3    
  4. 4    

The correct answer is: 3

Related Questions to study

General
Chemistry-

The product of the concentrations of the -ions of an electrolyte raised to power of their coefficients in the balanced chemical equation in the solution at any concentration. Its value is not constant and varies with change in concentration. Ionic product of the saturated solution is called solubility product K subscript s p end subscript
i) When K subscript i p end subscript equals K subscript S R end subscript ' the solution is just saturated and no precipitation takes place
ii) When K subscript i p end subscript less than K subscript S R end subscript the solution is unsaturated, and precipitation will not take place
iii) When K subscript i p end subscript greater than K subscript S R end subscript ' the solution is supersaturated, and precipitation takes place
Which of the following is most soluble?

The product of the concentrations of the -ions of an electrolyte raised to power of their coefficients in the balanced chemical equation in the solution at any concentration. Its value is not constant and varies with change in concentration. Ionic product of the saturated solution is called solubility product K subscript s p end subscript
i) When K subscript i p end subscript equals K subscript S R end subscript ' the solution is just saturated and no precipitation takes place
ii) When K subscript i p end subscript less than K subscript S R end subscript the solution is unsaturated, and precipitation will not take place
iii) When K subscript i p end subscript greater than K subscript S R end subscript ' the solution is supersaturated, and precipitation takes place
Which of the following is most soluble?

Chemistry-General
General
Chemistry-

An acid-base titration consists of the controlled addition of a dissolved base to a dissolved acid (or the reverse). Acid-base react rapidly to neutralize each other. At the equivalence point, enough titrant, the solution being added, has gone into make the chemical amounts of the acid and base' exactly equal. The pH of a titration changes every time a drop of titrant is added, but the rate of this change varies enormously. A titration curve, graph of pH tis a function of the volume of titrant, displays in detail how the pH changes over the course of an acid-base titration. Significantly, the pH changes most rapidly near the equivalence point. The exact shape of a titration curve depends on the K subscript a end subscript and K subscript b end subscript acid and base
Which of the titrations could it represent?

An acid-base titration consists of the controlled addition of a dissolved base to a dissolved acid (or the reverse). Acid-base react rapidly to neutralize each other. At the equivalence point, enough titrant, the solution being added, has gone into make the chemical amounts of the acid and base' exactly equal. The pH of a titration changes every time a drop of titrant is added, but the rate of this change varies enormously. A titration curve, graph of pH tis a function of the volume of titrant, displays in detail how the pH changes over the course of an acid-base titration. Significantly, the pH changes most rapidly near the equivalence point. The exact shape of a titration curve depends on the K subscript a end subscript and K subscript b end subscript acid and base
Which of the titrations could it represent?

Chemistry-General
General
Chemistry-

An acid-base titration consists of the controlled addition of a dissolved base to a dissolved acid (or the reverse). Acid-base react rapidly to neutralize each other. At the equivalence point, enough titrant, the solution being added, has gone into make the chemical amounts of the acid and base' exactly equal. The pH of a titration changes every time a drop of titrant is added, but the rate of this change varies enormously. A titration curve, graph of pH tis a function of the volume of titrant, displays in detail how the pH changes over the course of an acid-base titration. Significantly, the pH changes most rapidly near the equivalence point. The exact shape of a titration curve depends on the K subscript a end subscript and K subscript b end subscript acid and base
The following figure represents titration curve of HCl against NaOH. The pH at equivalence point will be:

An acid-base titration consists of the controlled addition of a dissolved base to a dissolved acid (or the reverse). Acid-base react rapidly to neutralize each other. At the equivalence point, enough titrant, the solution being added, has gone into make the chemical amounts of the acid and base' exactly equal. The pH of a titration changes every time a drop of titrant is added, but the rate of this change varies enormously. A titration curve, graph of pH tis a function of the volume of titrant, displays in detail how the pH changes over the course of an acid-base titration. Significantly, the pH changes most rapidly near the equivalence point. The exact shape of a titration curve depends on the K subscript a end subscript and K subscript b end subscript acid and base
The following figure represents titration curve of HCl against NaOH. The pH at equivalence point will be:

Chemistry-General
parallel
General
Chemistry-

When a salt reacts with water to form acidic or basic solution, the process is called hydrolysis. The pH of salt solution can be calculated using the following relations
p H equals fraction numerator 1 over denominator 2 end fraction open square brackets p K subscript w end subscript plus p K subscript a end subscript plus l o g invisible function application C close square brackets
(for salt of weak acid and strong base.)
p H equals fraction numerator 1 over denominator 2 end fraction open square brackets p K subscript w end subscript minus p K subscript b end subscript minus l o g invisible function application C close square brackets
(for salt of weak base and strong acid.)
p H equals fraction numerator 1 over denominator 2 end fraction open square brackets p K subscript w end subscript plus p K subscript a end subscript minus p K subscript b end subscript close square brackets
(for salt of weak acid and weak base.)
where, 'C' represents the concentration of salt.
When a weak acid or a weak base is not completely neutralized by strong base or strong acid respectively, then formation of buffer takes place. The pH of buffer solution can be calculated using the following relation
p H equals p K subscript a end subscript plus log invisible function application fraction numerator open square brackets blank S a l t blank close square brackets over denominator open square brackets blank A c i d blank close square brackets end fraction semicolon p O H equals p K subscript b end subscript plus log invisible function application fraction numerator open square brackets blank S a l t blank close square brackets over denominator open square brackets blank B a s e blank close square brackets end fraction
p K subscript a end subscript equals 4.7447 comma p K subscript b end subscript equals 4.7447 comma p K subscript w end subscript equals 14
When 50 mL of 0.1 M NaOH is added to 50 mL of 0.05 M C H subscript 3 end subscript C O O H solution. The pH of the solution is:

When a salt reacts with water to form acidic or basic solution, the process is called hydrolysis. The pH of salt solution can be calculated using the following relations
p H equals fraction numerator 1 over denominator 2 end fraction open square brackets p K subscript w end subscript plus p K subscript a end subscript plus l o g invisible function application C close square brackets
(for salt of weak acid and strong base.)
p H equals fraction numerator 1 over denominator 2 end fraction open square brackets p K subscript w end subscript minus p K subscript b end subscript minus l o g invisible function application C close square brackets
(for salt of weak base and strong acid.)
p H equals fraction numerator 1 over denominator 2 end fraction open square brackets p K subscript w end subscript plus p K subscript a end subscript minus p K subscript b end subscript close square brackets
(for salt of weak acid and weak base.)
where, 'C' represents the concentration of salt.
When a weak acid or a weak base is not completely neutralized by strong base or strong acid respectively, then formation of buffer takes place. The pH of buffer solution can be calculated using the following relation
p H equals p K subscript a end subscript plus log invisible function application fraction numerator open square brackets blank S a l t blank close square brackets over denominator open square brackets blank A c i d blank close square brackets end fraction semicolon p O H equals p K subscript b end subscript plus log invisible function application fraction numerator open square brackets blank S a l t blank close square brackets over denominator open square brackets blank B a s e blank close square brackets end fraction
p K subscript a end subscript equals 4.7447 comma p K subscript b end subscript equals 4.7447 comma p K subscript w end subscript equals 14
When 50 mL of 0.1 M NaOH is added to 50 mL of 0.05 M C H subscript 3 end subscript C O O H solution. The pH of the solution is:

Chemistry-General
General
Chemistry-

The equilibrium constant for this reaction is approximately 10 to the power of negative 3 end exponent H P O subscript 4 end subscript superscript 2 minus end superscript left parenthesis a q right parenthesis plus H C O subscript 3 end subscript superscript minus end superscript left parenthesis a q right parenthesis rightwards harpoon over leftwards harpoon H subscript 2 end subscript P O subscript 4 end subscript superscript minus end superscript left parenthesis a q right parenthesis plus C O subscript 3 end subscript superscript 2 minus end superscript left parenthesis a q right parenthesis Which is the strongest conjugate base in this reaction?

The equilibrium constant for this reaction is approximately 10 to the power of negative 3 end exponent H P O subscript 4 end subscript superscript 2 minus end superscript left parenthesis a q right parenthesis plus H C O subscript 3 end subscript superscript minus end superscript left parenthesis a q right parenthesis rightwards harpoon over leftwards harpoon H subscript 2 end subscript P O subscript 4 end subscript superscript minus end superscript left parenthesis a q right parenthesis plus C O subscript 3 end subscript superscript 2 minus end superscript left parenthesis a q right parenthesis Which is the strongest conjugate base in this reaction?

Chemistry-General
General
Chemistry-

If equal volumes of B a C l subscript 2 end subscriptand NaF solutions are mixed, which of these combinations will not give a precipitate?

If equal volumes of B a C l subscript 2 end subscriptand NaF solutions are mixed, which of these combinations will not give a precipitate?

Chemistry-General
parallel
General
Chemistry-

The amount of sodium hydrogen carbonate, N a H C O subscript 3 end subscript, in an antacid tablet is to be determined by dissolving the tablet in water and titrating the resulting solution with hydrochloric acid Which indicator is the most appropriate for this titration?

The amount of sodium hydrogen carbonate, N a H C O subscript 3 end subscript, in an antacid tablet is to be determined by dissolving the tablet in water and titrating the resulting solution with hydrochloric acid Which indicator is the most appropriate for this titration?

Chemistry-General
General
Chemistry-

The correct order of basic strength is

The correct order of basic strength is

Chemistry-General
General
Chemistry-

4Three sparingly soluble salts that have same solubility products are given below:
∣ A subscript 2 end subscript X
II A X
III A X subscript 3 end subscript
Their solubilities in a saturated solution will be such that:

4Three sparingly soluble salts that have same solubility products are given below:
∣ A subscript 2 end subscript X
II A X
III A X subscript 3 end subscript
Their solubilities in a saturated solution will be such that:

Chemistry-General
parallel
General
Chemistry-

A) The aqueous solution of C H subscript 3 end subscript C O O N a is alkaline in nature.
R) Acetate ion undergoes an ionic hydrolysis

A) The aqueous solution of C H subscript 3 end subscript C O O N a is alkaline in nature.
R) Acetate ion undergoes an ionic hydrolysis

Chemistry-General
General
Chemistry-

A) At 25 to the power of ring operator end exponent C, the pH of 10 to the power of negative 8 end exponentM HCl is 8.
R) pH of acidic solution is always below 7 at 25 to the power of ring operator end exponent C

A) At 25 to the power of ring operator end exponent C, the pH of 10 to the power of negative 8 end exponentM HCl is 8.
R) pH of acidic solution is always below 7 at 25 to the power of ring operator end exponent C

Chemistry-General
General
Chemistry-

A) When small amount of an acid or base is added to pure water its pH undergoes a change
R) Addition of an acid or a base increases the degree of ionization of water

A) When small amount of an acid or base is added to pure water its pH undergoes a change
R) Addition of an acid or a base increases the degree of ionization of water

Chemistry-General
parallel
General
Chemistry-

The weak acid, HA has a K subscript a end subscript of 1.00 cross times 10 to the power of negative 5 end exponent. If 0.1 text end text m o l of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closet to:

The weak acid, HA has a K subscript a end subscript of 1.00 cross times 10 to the power of negative 5 end exponent. If 0.1 text end text m o l of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closet to:

Chemistry-General
General
Chemistry-

The ionization constant of ammonium hydroxide is 1.77 cross times 10 to the power of negative 5 end exponent at 298 text end text K. Hydrolysis constant of ammonium chloride is:

The ionization constant of ammonium hydroxide is 1.77 cross times 10 to the power of negative 5 end exponent at 298 text end text K. Hydrolysis constant of ammonium chloride is:

Chemistry-General
General
Chemistry-

The molar solubility (in mol text  litre  end text to the power of negative 1 end exponent) of a sparingly soluble salt M X subscript 4 end subscript is The corresponding solubility product K subscript s p end subscript is given by the relation

The molar solubility (in mol text  litre  end text to the power of negative 1 end exponent) of a sparingly soluble salt M X subscript 4 end subscript is The corresponding solubility product K subscript s p end subscript is given by the relation

Chemistry-General
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