ZuoTi.Pro
Question

11. Consider the following chemical equation that describes the titration between Ag+ and Cl −; Ag+...

11. Consider the following chemical equation that describes the titration between Ag+ and Cl −;

Ag+ (aq) + Cl − (aq) → AgCl (s)

When adding Ag+ to Cl −, the equivalence point is reached when:

A) no more AgCl can precipitate from solution.

B) an excess of Ag+ has been added.

C) Cl − has just started to be consumed by Ag+.

D) half of the Cl − is consumed by Ag+.

E) none of the above happens.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)

All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
11. Consider the following chemical equation that describes the titration between Ag+ and Cl −; Ag+...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Similar Homework Help Questions

  • 2.         The Ka of nitrous acid HNO2is 4.5 x 10-4.  In a titration, 50.0 mL of 1.00 M...

    2.         The Ka of nitrous acid HNO2is 4.5 x 10-4.  In a titration, 50.0 mL of 1.00 M HNO2is tit  rated with 0.750 M NaOH.                  a. Calculate the pH of the solution:                         (i) Before the titration begins. (ii) When sufficient NaOH has been added to neutralize half the nitrous acid                   originally present.                         (iii) At the equivalence point. (iv)When 0.05 mL NaOH less than that required to reach the equivalence point  has been added. (v) When 0.05 mL NaOH more than that required to reach the...

  • No clue for any of the following questions. In Ms experiment, dissociation of KHP occurs in...

    No clue for any of the following questions. In Ms experiment, dissociation of KHP occurs in solution as shown on p. 32 in the Laboratory Manual. Similarly, which of the following accurately depots the balanced dissociation reaction of formic acid (CH_3COOH) in water? CH_3COOHM rightarrow CH_3CO^+(aq) + OH^-(aq) CH_3COOH(ap) rightarrow CH_3COO(aq) + H(aq) CH_3COOH(aq) rightarrow CH_3COO^-(aq) + H^+(aq) all of the above are accurate When a base of known concentration is added to an acid of unknown concentration, which is...

  • Account for your observations. Consider the following equilibria: Ag^+(aq)+Cl^-(aq)<->AgCl(s) Ag^+(aq)+2NH3(aq)<->[Ag(NH3)2]^+(aq) NH3(aq)+H^+(aq)<->NH4^+(aq) Observations:    adding NaCl: went...

    Account for your observations. Consider the following equilibria: Ag^+(aq)+Cl^-(aq)<->AgCl(s) Ag^+(aq)+2NH3(aq)<->[Ag(NH3)2]^+(aq) NH3(aq)+H^+(aq)<->NH4^+(aq) Observations:    adding NaCl: went from clear to a white solution adding NH3: went from white solution to. clear solution adding HNO3: solution warmed up

  • Consider the reaction Fe3+(aq) + Cl-(aq)   FeCl2+(aq). If Ag+(aq) is added, the silver ion will react with...

    Consider the reaction Fe3+(aq) + Cl-(aq)   FeCl2+(aq). If Ag+(aq) is added, the silver ion will react with (Cl-, H2O, Fe3+) to form a precipitate, which will (decrease, increase, or not change) the concentration of reactants and drive the reaction(to the left, to the right, or neither one way or the other). When this happens, the value of Kc will be(lower, higher, or constant).

  • In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion,...

    In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...

  • The value of the equilibrium constant for the following chemical equation is Kc = 5.2 ×103...

    The value of the equilibrium constant for the following chemical equation is Kc = 5.2 ×103 AgCl (s) + 2S2O32-<-->[Ag(S2O3)2]3- (aq) + Cl– (aq) Calculate the solubility of AgCl (s) in an aqueous solution whose equilibrium concentration of S2O32- is 0.015 M. Ksp = 1.8 × 10-10 M2 for AgCl

  • consider the titration of a weak monoprotic acid (HA) with a strong base. If the titration...

    consider the titration of a weak monoprotic acid (HA) with a strong base. If the titration has begun, but the equivalence point has not yet been reached, which of the following is true: A) The solution is a bugger and the HH equation can be used to compute the solution pH B) The excess titrant will dominate and control the pH at this point C) The dissociation of the weak acid to donate protons will determine pH - make a...

  • 1. Consider two nearly insoluble silver salts, silver chlor FINAL Equilibrium Practice Set molar solubility of...

    1. Consider two nearly insoluble silver salts, silver chlor FINAL Equilibrium Practice Set molar solubility of AgCl is 1.3 E-5. The molar solubility of AgaC puble silver salts, silver chloride, AgCl, and silver chromate, AgzCros. The E-5. The molar solubility of AgaCrocis 1.3 E-4. a. Write the the chemical equation for the solubility equilibrium of AgCl. What is the Ksp value for AgCl? b. Write the chemical equation for the solubility equi chemical equation for the solubility equilibrium of AgaCros....

  • Another form of this equation (called the complete ionic equation) indicates the species that are actually...

    Another form of this equation (called the complete ionic equation) indicates the species that are actually present in solution. 2Na+ + CO32-+2hr + 2 cr . 4 co2 +H2O + 2 Na. + 2 cr Since balanced chemical equations indicate only substances that change, this equation simplifies to This simplified equation is called a net ionic equation. The evolution of CO2 gas is visible as tiny bubbles. Sulfate, so2 Sulfate, So,, is found in compounds such as NaSO4. If a...

  • Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium...

    Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT