Write balanced chemical equation for the given reactions and also predict whether precipitate will form or not. NaBr ( aq ) + AgNO 3 ( aq ) Concept introduction: Precipitation reaction takes place when anions and caations present in the solution combine to form insoluble salt. The salt will be soluble or insoluble depends upon the K sp value of the salt. Higher the K sp value soluble will be the salt. Salts having lower K sp value are insoluble or dissolve very less in water. Generally chlorides, bromides, iodides of Ag + , Pb 2+ and Hg 2 2+ are insoluble whereas nitrates are soluble.
Write balanced chemical equation for the given reactions and also predict whether precipitate will form or not. NaBr ( aq ) + AgNO 3 ( aq ) Concept introduction: Precipitation reaction takes place when anions and caations present in the solution combine to form insoluble salt. The salt will be soluble or insoluble depends upon the K sp value of the salt. Higher the K sp value soluble will be the salt. Salts having lower K sp value are insoluble or dissolve very less in water. Generally chlorides, bromides, iodides of Ag + , Pb 2+ and Hg 2 2+ are insoluble whereas nitrates are soluble.
Solution Summary: The author explains that precipitation reaction takes place when anions and caations present in the solution combine to form insoluble salt.
Interpretation: Write balanced chemical equation for the given reactions and also predict whether precipitate will form or not.
NaBr(aq)+AgNO3(aq)
Concept introduction: Precipitation reaction takes place when anions and caations present in the solution combine to form insoluble salt. The salt will be soluble or insoluble depends upon the Ksp value of the salt. Higher the Ksp value soluble will be the salt. Salts having lower Ksp value are insoluble or dissolve very less in water.
Generally chlorides, bromides, iodides of Ag+, Pb2+ and Hg22+ are insoluble whereas nitrates are soluble.
(b)
Interpretation Introduction
Interpretation: Write balanced chemical equation for the given reactions and also predict whether precipitate will form or not.
KCl(aq)+Pb(NO3)2(aq)
Concept introduction: Precipitation reaction takes place when anions and caations present in the solution combine to form insoluble salt. The salt will be soluble or insoluble depends upon the Ksp value of the salt. Higher the Ksp value soluble will be the salt. Salts having lower Ksp value are insoluble or dissolve very less in water.
Generally chlorides, bromides, iodides of Ag+, Pb2+ and Hg22+ are insoluble whereas nitrates are soluble.
The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows:
HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l)
Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH.
1. what is the pH when the volume of base added equals half the volume of the equivalence point?
2. what is the pH of the titration when 20.00 mL of base have been added?
3. what is the pH of the titration when 30.00 mL of base have been added?
A saturated solution of Cd(OH)2 is shown in the middlebeaker. If hydrochloric acid solution is added, the solubilityof Cd(OH)2 will increase, causing additional solid to dissolve. Which of the two choices, Beaker A or Beaker B,accurately represents the solution after equilibrium is reestablished?(The water molecules and CI- ions are omittedfor clarity.)
(5) a) A nitrous acid/sodium nitrite buffer solution is prepared. 20.0 mL of 6.50 M nitrous acid (HNO2) and 8.52 g of sodium nitrite (NaNO2, molar mass 68.99 g/mol) are placed in a 250. mL volumetric flask. The flask is filled to the mark with water and inverted 10 times to mix thoroughly. What is the pH of this buffer? Take Ka for Nitrous Acid to be 4.52 x 10-4.
pH:
b) 2.00 mL of a 2.50 M solution of NaOH is added to 75.0 mL of the buffer prepared above. What is the pH of this solution? How much did the pH change?
pH: change in pH:
c) What is the pH of pure distilled water (just give the pH, no calculations are necessary).
d) If 2.00 mL of 2.50 M…
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell