2. Write an equation showing the dissolution reaction for each of the precipitates that was soluble inCH;COOH solution.LAB 5: NET IONIC EQUATIONS 53 C.INSTRUCTORLOCKERSECTIONNAMENAMESECTIONLOCKERINSTRUCTORDATA SHEET 1DATA SHEET 2Naz CO3 Ala(5oa)II. Studying the Reactions of Unknown 2 30 VO3T01. Studying the Reactions of Known Solutions:- ClearOBSERVATIONSOBSERVATIONSSolutionSolution34XXPale SWhi teXX1XXNaCIDistincwhiePardicinsWhitParticksVeryMilkXXXXNOIO3 CWhite(IPartalesPale OwhileXXBaClaVar yA,VeryMilkyWhi keXXwhiteGranVeryPale4PaleNa, CO MilkyDistincwhiteParticlesXXVeryBacl5MlkwhitXXwhiteVery Pale MilkyWhitwhitePartichPaleXXorandeasesS: SoluableI: InslabeW/ whiteonXX6edsesChunksS: SolvableI: Insoluoble0 nominCHC

The given compounds dissolve in acetic acid and ionic reaction that takes place -

Answered: 2. Write an CH;COOH solution. equation…

2. Write an CH;COOH solution. equation showing the dissolution reaction for each of the precipitates that was soluble in

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: When K,So,(aq) and Pb(NO,),(aq) are mixed, a white colored precipitate forms which is Select one: a.…

A: Write reaction and determine the precipitate.

Q: Is KOH soluble or non soluble

A: Solublity: It is ability to dissolve a substance in given solution. Solublity depends upon polarity…

Q: Solid Nal is slowly added to a solution that is 0.0083 M Cu* and 0.0091 M Ag". Which compound will…

A: Given data,Molarity of Cu+=0.0083MMolarity of Ag+=0.0091MKsp of AgI=1.5 ×10-16(taken from google)Ksp…

Q: white precipitate forms. What are the cations that may be present in the precipitate? a) Addition of…

A: Group I cations precipitate on addition of aq. HCl. The group I cations form white precipitates. The…

Q: What is the pH at the equivalence point in the titration of a 17.0 mL sample of a 0.303 M aqueous…

A: We will first calculate the volume of Ba(OH)2. and since we need the total volume. and we will…

Q: Which of the following aqueous solutions would you expect CaF, (s) to have the lowest solubility? a)…

A: Which of the following aqueous solutions would you expect CaF₂ (s) to have the lowest solubility?

Q: 8. What color reactions are expected at the end of the equivalence point?

A: ALL THREE IS A PRECIPITATION TITRATION SILVER ION IS COMMON IN ALL THREE

Q: A 50.0 mL of 0.02 F ammonia solution is added to a solution containing 0.004 g Ni2, 0.003 g Mn2, and…

Q: B. Molar Solubility of Calcium Hydroxide in the Presence of a Common Ion Trial 1 Trial 2 Trial 3 1.…

A: 5.) Volume of HCl added is calculated using formula : Volume of HCl added (mL ) = Final buret…

Q: Arrange the salts by their molar solubility in water. value for Most soluble Least soluble

Q: 16 What weight of sample which contains 56.15 per cent Cl was taken for analysis if the precipitated…

A: Given data : Reaction undergoing in analysis , Ag+ + Cl- -----------> AgCl(s) weight of AgCl…

Q: The solubility product for an insoluble salt with the formula M2X3 is written as ________, where s…

A: Solubility product Ksp is the ratio of the equilibrium concentrations of product over equilibrium…

Q: An aqueous solution is prepared to be 0.261 M in sodium formate and 0.155 M in acetic acid. (1) Is…

Q: Sulfate precipitating

A: One factor is temperature, precipitation of sulfate ion is temperature dependent means when…

Q: A saturated solution of Al(OH), has a molar solubility of 6.5×10$ M at a certain temperature. What…

A: Solubility of any salt is defined as the maximum amount of solute that can be dissolve in a solvent…

Q: Determine the minimum concentration of the precipitating agent on the right to cause precipitation…

Q: The maximum amount of silver chromate that will dissolve in a 0.213 M sodium chromate solution is

A: Dear student, the value of the solubility product constant ksp of silver chromate is not mentioned,…

Q: what is a good example of introduction of the experiment "Determination of %SO3 in a Soluble Sample"

A: The amount of an analyte can be determined through the measurement of mass in the technique call…

Q: lodide Titrations Which of the following statement(s) regarding the triiodide standard used in…

A: Solution : Iodide titration defined as that titration where one oxidizing agent liberates iodine…

Q: Most soluble Fe(OH)3 BaSO, Mg(OH), Mg, (PO,), Least soluble Answer Bank

A: Solubility of any compound is measured in terms of their solvation energy and lattice energy.…

Q: 1. How many mL of 0.256M Al,(SO,); must be added to 175 ml of 0.154M Mg,(SO,), solution to make a…

A: Number of mmol = Molarity x Volume (mL) Number of mmol of SO42- released by 1 mmol of Al2(SO4)3 = 3…

Q: One of the main components of hard water is CaCo,. When hard water evaporates, some of the CaCO, is…

A: Given, 1.00 × 102 mg of CaCO3

Q: The molar solubility of calcium carbonate in a 0.269 M calcium acetate solution is ______________ M.

A: Given that: [Ca(CH3COO)2] = 0.269M Ca(CH3COO)2 .....> Ca2+(aq) + 2CH3COO-(aq) [Ca2+] = 0.269M

Q: 9. How does acid-base titration differ from precipitation titration?

Q: If OH is added to a solution containing 1.2 g ol Mg?' and 1.28 g of Cu? per liler, which lon will…

Q: 2. A saturated solution of an unknown solid reacted with AgNO, to give a pale yellow precipitate,…

A: The unknown anion is Bromine which when reacted with the AgNO3 and gives pale yellow precipitate and…

Q: Balance each of the following word equations. Find if the substances are soluble (aq) or insoluble…

Q: What's the value of solubility product constant for zinc phosphate?

A: Here are some of the references for the solubility product constant of zinc phosphate at 25oC:…

Q: The molar solubility of calcium carbonate in a water solution is M.

A: Using the ksp value and it's equation to calculate solubility.

Q: Acidic buffers consist of: a. a weak acid and a salt, that formed from a weak acid and a strong…

Q: When 20.00 mL of 0.1752 M sodium hydroxide is titrated with 0.2013 M sulfurous acid what volume of…

A: During titration, MacidVacid=MbaseVbase Given, MH2SO4=0.2013 M, MNaOH=0.1752 M and VNaOH=20 mL

Q: 7. Define back-titration. What is the concept behind this method?

A: Back titration; It is a titration method where the concentration of unknown sample is determined by…

Q: What are/is the disadvantage(s) of using iodine solution as a titrant? A Iodine can sublime. B odine…

A: The correct option is (D) Iodine can sublime at room temperature and at high temperatures,…

Q: Explain why some precipitates do not dissolve once formed with HCl. Explain by showing some examples

A: A question based on solutions that is to be accomplished.

Q: . a. In a lab project, a student obtained a highly turbid acidic solution whose concentration has to…

A: One of the methods by which we can determine the concentration of highly turbid acidic solution is…

Q: 10.0 ml 0.010M Na;CO, is combined with 10.0 mL 0.010 M AGN0,. a. What, if anything, precipitates…

A: Given: Concentration of Na2CO3 = 0.010 M Volume of Na2CO3 solution = 10.0 mL = 0.010 L…

Q: A chemistry graduate student is glven 250. mL of a 0.80M pyridine (C,H,N) solutlon. Pyridine Is a…

A: The Henderson Hasselbalch equation is - pH = pKb + log ([Salt]/[Base]) Here - pH = 5.43 pKb = -…

Q: e maximum amount of

Q: " The endpoint of an acid-base titration is defined as the point where. O A. The amount (moles) of…

A: End point is defined as.

Q: Which statement regarding lon Product (IP) and Solubility Products (K„) is CORRECT? A. When K, is a…

Q: 3. Is it possible to have a reaction in which oxidation occurs and the reduction does not? Explain.…

A: If a species/element losses electron then it will be a oxidation reaction. If a species/element…

Q: a. Give the chemical equation for the dissociation of Al(OH)3. 3. b. What is the molar solubility of…

A: The compound given is Al(OH)3.

Q: Solid calcium nitrate is slowly added to 50.0 mL of a ammonium fluoride solution until the…

Q: Solid nickel(II) hydroxide and solid nickel(II) cyanide are in equilibrium with a solution…

A: The solubility of given salts is shown as- Ni(OH)2⇔Ni2+(aq) + 2OH- (aq)…

Q: An unknown solution is titrated with a strong titrant. The pH at the equivalence point is 5.7. What…

A: Given, Unknown solution is titrated with strong titrant. pH at equivalence point = 5.7

Question

100%

2. Write an equation showing the dissolution reaction for each of the precipitates that was soluble in
CH;COOH solution.
LAB 5: NET IONIC EQUATIONS 53

C.
INSTRUCTOR
LOCKER
SECTION
NAME
NAME
SECTION
LOCKER
INSTRUCTOR
DATA SHEET 1
DATA SHEET 2
Naz CO3 Ala(5oa)
II. Studying the Reactions of Unknown 2 30 VO3T0
1. Studying the Reactions of Known Solutions
:- Clear
OBSERVATIONS
OBSERVATIONS
Solution
Solution
3
4
XX
Pale S
Whi te
XX
1
XX
NaCI
Distinc
whie
Pardicins
Whit
Particks
Very
Milk
XX
XX
NOIO3 C
White(I
Partales
Pale O
while
XX
BaCla
Var yA,
Very
Milky
Whi ke
XX
white
Gran
Very
Pale
4
Pale
Na, CO Milky
Distinc
white
Particles
XX
Very
Bacl
5
Mlk
whit
XX
white
Very Pale MilkyWhit
white
Partich
Pale
XX
orand
eases
S: Soluable
I: Inslabe
W/ white
on
XX
6
edses
Chunks
S: Solvable
I: Insoluoble
0 nom
inCHC

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

In chlorides of alkaline earth metals solubility decreases down the group why? Plz explain briefly
Please answer questions 3a&b based on the information in question 2.
Suppose that when the saturated solution was generated there was no precipitate observed and the solution was not filtered before starting the titration. Explain how not having a precipitate in the saturated solution affects the results. Be specific about how the calculated molarity of the hydrogen tartrate ion is affected. Edit View
presented by Macmilan Learning The acetic acid/acetate buffer system is a common buffer used in the laboratory. To prepare an acetic acid/acetate buffer, a technician mixes 30.7 ml. of 0.0951 M acetic acid and 20.1 ml. of 0.112 M sodium acetate in a 100 mL volumetric flask and then fills with water to the 100 ml. mark. How many moles of acetic acid are present in this buffer? acetic acid: mol How many moles of sodium acetate are in the buffer? sodium acetate: mol
Which of the following would keep the relative super saturation high during precipitation? 1. O Elevated temperature. 2. O Adding concentrated solutions. 3. O Slow addition of precipitating agent with good stirring. 4. OAll of the above.
Is copper(II) iodide A. Soluble B. Not soluble
4. Two RND Engineers were assigned to create buffer solutions for two separate product lines that were susceptible to degradation if their pH was not maintained at a certain level. [a.] Engr. Baylon prepared the buffer for the product that requires a pH of around 4.0 by mixing 0.225 M of phosphoric acid and 0.414 M of sodium dihydrogen phosphate [b.] 0.640 M of ethanolamine, HOC,H,NH, were mixed with 0.750 M of its chloride salt, HOC,H4NH3CI, by Engr. Samonte for the alkali goods that requires a pH of 9.5 max. Are the prepared buffers solutions applicable for their intended use? Take the acid ionization constant of phosphoric acid to be 7.1x10-3 while the base ionization constant of ethanolamine is 2.68x10-5
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
For metal ions that do not have a good indicator, a second titration method is the direct titration. is it t or f?
all 3 parts please
If during the titration a drop of the standardized NaOH adhered to the side of the Erlenmeyer flask and did not enter the vinegar solution would this result in a percent acetic acid that is too high, too low or would it have no effect? Explain
A solution containing 10. mmol of and 5.0 mmol of is titrated with 1.5 M HCl. What total volume of HCl must be added to reach the second equivalence point? a. 6.7 mL b. 10.0 mL c. 3.3 mL d. 16.7 mL e. 21.7 mL