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September 1, 2014

Search: if 10 mL of 0.004M AgNO3 is added to 10mL of 0.0024M K2CrO4, is eitheR Ag+ or CrO42- in stoichiometric excess? if so, which is in excess?

Number of results: 9,604

chemistry
1. if 10mL of 0.004M AgNO3 is added to 10mL of 0.0024M K2CrO4, is either Ag+ or CrO4(2-) in stoichiometric excess? if so, which is in excess? 2. the Ksp for BaCrO4 is 1.2x10-10. will BaCrO4 precipitate upon mixing 10 mL of 1x10-4M Ba(NO3)2 with 10mL of 1.0x10-4M K2CrO4?
October 19, 2009 by millie

Chemistry
Calculate the number of moles of ag in 5ml of .004m agno3 and the number of moles of cr04 in 5ml of .0024m k2cro4
March 19, 2014 by Candice

ap
An excess of aqueous AgNO3 reacts with 44.5 mL of 5 M K2CrO4(aq) to form a precip- itate. What is the precipitate? 1. K2CrO4 2. KNO3 3. Ag2CrO4 4. AgNO3
October 1, 2012 by cheri

Chemistry
An excess of aqueous AgNO3 reacts with 24.5 mL of 5 M K2CrO4(aq) to form a precip- itate. What is the precipitate? 1. AgNO3 2. Ag2CrO4 3. KNO3 4. K2CrO4
October 14, 2010 by John

ap
An excess of aqueous AgNO3 reacts with 44.5 mL of 5 M K2CrO4(aq) to form a precip- itate. What is the precipitate? 1. K2CrO4 2. KNO3 3. Ag2CrO4 4. AgNO3 What mass of precipitate is formed? Answer in units of g
October 1, 2012 by cheri

Electrochemistry
Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a silver wire coated ...
May 20, 2008 by Daniel

George School
Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a silver wire coated ...
May 20, 2008 by Daniel

chemistry
mix 10ml NaBr 3.i000M wth 10ml water & 10ml AgNo3 3.3.1000M KspAgBr=5.25.1000 .what is the situation at equilibrium
November 22, 2011 by rene

Chem 22
molecular equation, and net ionic equation of K2SO4 + MgCl2 NiCl2 + NaOH MgCl2 + NaOH K2SO4 + NaOH Ba(OH)2 + NiCl2 Ba(OH)2 + MgCl2 Ba(OH)2 + K2SO4 Ba(OH)2 + NaOH Na2CrO4 + Sr(NO3)2 Na2CrO4 + Al2(SO4)3 K2CrO4 + Sr(NO3)2 K2CrO4 + Al2(SO4)3 AgNO3 + BaCl2 AgNO3 + Na2CrO4 AgNO3 + ...
December 3, 2010 by Anonymous

chemistry
A solution of AgNO3 (1 x 10-6 molar) is prepared. To this is added K2CrO4 until precipitation of Ag2CrO4 begins. The Ksp of Ag2 CrO4 is 9 X 10-12. Addition of NaCl will bring about:
January 14, 2011 by shahanas

Science(Chemistry)
Suppose that 23 mL of 0.6 M K2CrO4(aq) reacts with 13.7 mL of AgNO3(aq) completely. What mass of NaCl is needed to react completely with 38.5 mL of the same AgNO3 solution? Answer in units of g
April 18, 2013 by Joseph

chemistry
By means of what single reagent could you distinguish between the following? (Tell what happens to each substance.) Solutions: AgNO3 and Zn(NO3)2 H2SO4 and HNO3 Ag(NH3)2Cl and AgNO3 Solids: AgCl and ZnCl2 AgCl and Hg2Cl2 PbCrO4 and K2CrO4
February 4, 2010 by Becky

Chemistry
Net ionic equations for: Br- + AgNO3 CO3 + AgNO3 Cl-+ AgNO3 I + AgNO3 PO4^-3 + AgNO3 SO4^-2 + AgNO3 S^-2 + AgNO3 They all formed ppt,but I don't know where to go from here. Even a couple to get me started would be greatly appreciated!
July 14, 2013 by Ann

chemistry
Calculate the molarity (mol/L) of Ba2+ when BaCrO4 is placed in a 0.0457 M K2CrO4 solution. The equation represents the solubility process. K(sp)=1.2x10^-10 BaCrO4 (s) Ba2+ (aq) + CrO42- (aq)
April 14, 2010 by bme1

Chemistry
What volume of 0.123 M NaOH(aq) must be added to 125 mL of 0.197 M H2SO3(aq) to reach the following points? (a) the first stoichiometric point (b) the second stoichiometric point
June 14, 2013 by Sara

Chemistry
What volume of 0.123 M NaOH(aq) must be added to 125 mL of 0.197 M H2SO3(aq) to reach the following points? (a) the first stoichiometric point (b) the second stoichiometric point
June 14, 2013 by Sara

chemistry
What is the concentration of this solution? If you added 10mL of water to the 10mL of 0.010M CaCl2 solution.
September 13, 2010 by fredy

chemistry
There is a titration of 5.00 mL .010 M NaOH with .005 M HCl. Indicate the pH of the initial and final solutions and the pH at the stoichiometric point. What volume of HCl has been added at the stoichiometric point and the halfway point of the titration? I have no idea how to ...
December 3, 2011 by Betty

Chemistry
How many milliliters of 0.645 M K2CrO4 are needed to precipitate all the silver in 405 mL of 0.190 M AgNO3 as Ag2CrO4?
February 19, 2011 by Abigail

Chemistry Help!!!!!
How many milliliters of 0.635M K2CrO4 are needed to precipitate all the silver in 410mL of 0.158M AgNO3 as AgCrO4 ?
February 25, 2013 by Lisa

college chemistry
How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer + 5mL water + 1mL ...
April 13, 2009 by Mary

college chemistry
How do you calculate the pH difference when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer + 5mL ...
April 13, 2009 by Mary

Chemistry- Le chatelier's Principle
HOw would you predict the colour change or changes in number of states for the following: To a solution of 5 drops of 0.3 M K2CrO4 ans 2 drops of 0.3M NaOH add a drop at a time 0.1 M Ba(NO3)2 until a change is noticed. Given: BaCrO4(s) ---> Ba2+ + CrO42- 2CrO42-+2H+ --->...
March 4, 2009 by meme

college
A solid is known to be either BaCO3 or CaCO3. It is dissolved in 6 M acetic acid. A pale yellow precipitate forms when K2CrO4 solution is added. The subsequent flame test with that precipitate shows an orange-red color. Which cation is present? Briefly explain
March 22, 2013 by Anonymous

Chemistry
Even if you can help answer one that would be a great help! 1. How many liters of NO(g) are produced when 0.85L of 2.00M HNO3 solution is added to 216g according to the equation. Which reactant is the limiting reactant? 3 Ag + 4 HNO3 -> 3 AgNO3 + NO + 2 H2O3 2. Calculate ...
October 20, 2013 by P.

chemistry
How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer + 5mL water + 1mL ...
April 14, 2009 by Mary

organic chemistry
Partition (distribution) coefficient, k, of benzyl alcohol in hexane and water is 12.0. Choose for the correct equation for the amount of benzyl alcohol as x that you should use to calculate the amount of benzyl alcohol extracted with one 10mL portion of hexane from 500mg of ...
November 25, 2008 by Jenn

chemistry
An excess of aqueous AgNo3 reacts with 41 mL of 5 M K2CrO4(aq) to form a precipitate. What is the precipitate?
December 12, 2013 by Anonymous

Chemistry
1.Calculate the pH of a solution prepared by mixing 20mL of the .07222M aspirin solution with 10mL of .2M NaOH. 2. Calculate the pH for the titration of 40mL of .1M solution of C2H5NH2 with .1M HCl for a)0 mL added and b)20 mL added c)40 mL added d)50mL added. Kb= 6.4x10^-4
November 26, 2011 by Jessica

Chemistry (AP)
5 drops of AgNO3 must be added to 1 L of a water sample: 46.1 mg SO42-/L and 30.6 mg Cl -/L. What will be the precipitate that forms? the molarity of AgNO3 is 0.0010 M (mol/L) 1 drop = 0.05 mL
April 22, 2010 by Tommy

Chemisty
An excess of aqueous AgNO3 reacts with 43 mL of 5 M K2CrO4(aq)to form a precipitate. what is it? What mass of precipitate is formed? answer in g
February 9, 2014 by Anonymous

Chemisty
Please help...I know I'm missing something here if 50.0mL of AgNO3 reacts with 25.0mL of 0.100M of K2CrO4, what is the molarity of silver nitrate?
August 10, 2012 by Sheri

chemistry
In a particular redox reaction, Cr is oxidized to CrO42 and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution. Phases are optional. Cr + Cu2+ = CrO42- + Cu+
February 24, 2012 by Anonymous

math
A phsician orders 750mg of chloramphenicol to be added to a 100ml bag os NS. if the drug is reconstituted to 1gm/10ml, how many mls will be added to the NS?
January 25, 2010 by crystal

Chemistry
at 23C the reaction CaCrO4 -> Ca2+ + CrO42- has an equilibrium constant of 7.1 x 10-4. what are the equilibrium concentrations of Ca2+ and CrO42- in a saturated solution?
March 22, 2010 by Ry

chemistry
A solution prepared by mixing 16.7 mL of 0.760 M NaCl and 16.7 mL of 0.760 M KI was titrated with 0.380 M AgNO3 in a cell containing a silver indicator electrode and a saturated calomel reference electrode. (a) What is [Ag+] when 16.2 mL of 0.380 M AgNO3 have been added? ...
March 11, 2014 by Bobz

MATH HELP PLZ
A physician orders 750mg of chloramphenicol to be added to a 100ml bag of NS. If the drup is reconstituted to 1gm/10ml, how many mills will be added to NS?
February 16, 2012 by Vicki

Chemistry
how many grams of each species will be present at the end when 0.500g of copper is added to 2.500g of AgNO3? Cu(s) + 2 AgNO3(aq) --> 2 Ag(s) + Cu(NO3)2 (aq)
June 8, 2011 by tc

Chemistry
A solution of K2CrO4 was titrated with AgNO3, using a silver indicator electrode (E=0.799V) and a S.C.E. electrode (E=0.241V). The product, Ag2CrO4, has a Ksp = 1.1x10^-12. What is the potential at the equivalence point?
May 28, 2012 by Jeanie

chem
For a mixture of 12.0mL of 0.004. M AgNO3 and 8.0mL of 0.0025 M K2CrO4, a colorimetric measurement of CrO4-2 in the equilibrium supernatant liquid found its concentration to be 1.5*10^-4 M. Calculate the Ksp of Ag2CrO4.
July 9, 2012 by jerry

Chemistry
For the following Reaction: 2AgNO3 + CaBr2 = 2AgBr + CaN2O6 If a chemist starts with 12.0g AgNO3, how many grams of CaBr2 must be added to use up all of the AgNO3?
November 14, 2011 by Carrie

Chemistry
This is a limit test for chlorides. 1.0g of NaOH sample was dissolved in 5ml of deionized water, acidified with 4ml of concentrated nitric acid (65%) and diluted to 15ml with deionized water. (Test tube A) 10ml of 50ppm Standard NaCl solution was prepared. 5ml of water was ...
September 24, 2010 by candy

Chemistry
If you mix 40.0 mL of a 0.389 M solution of K2CrO4 with 40.0 mL of a 0.389 M solution of AgNO3, what mass of solid forms?
November 20, 2010 by Angela

chem
mix 35.50 mL of a 0.201 M solution of K2CrO4 with 35.50 mL of a 0.201 M solution of AgNO3, what mass of solid will form?
November 29, 2011 by darren

Chemistry
To 40cm^3 of 1mol AgNO3 is added 20cm^3 of 0.500 AlCl3. What is the molar concentration of the resulting AgNO3 solution. The reaction, if needed, is 3AgNO3 + AlCl3 ==> 3AgCl + Al(NO3)3 I worked out the number of moles present in AgNO3 which is 0.04 mol, and the number of ...
December 30, 2012 by Matt

science(chem)
I'm making different concentrations of ethanol and I just wanted to check my calculations and method. Making ethanol concentrations of: 0.40% 0.30% 0.20% 0.10% 0.05% To make the 0.40% ethanol from stock solution using 100ml volumetric flask: (xg ethanol)/(100ml) x 100= 0.40% ...
October 1, 2008 by ~christina~

Chemistry
An excess of aqueous AgNO3 reacts with 24.5 mL of 5 M K2CrO4(aq) to form a precipitate. What is the precipitate? Answer: Ag2CrO4 What mass of precipitate is formed? Answer in units of g.
March 23, 2011 by Mary

Chemistyr
BaCl2(aq) + K2CrO4(aq) BaCrO4(s) + 2 KCl(aq) How many milliliters of 0.1200 M K2CrO4(aq) will react with 0.045 mol of BaCl2(aq)?
February 23, 2011 by Anonymous

Chemistyr
BaCl2(aq) + K2CrO4(aq) BaCrO4(s) + 2 KCl(aq) How many milliliters of 0.1200 M K2CrO4(aq) will react with 0.045 mol of BaCl2(aq)?
February 23, 2011 by Anonymous

chemistry
Balance the redox reactin in basic. ClO- + Cr(OH)4- --> CrO42- + Cl- H2O + ClO- --> Cl- + 2OH ClO- has a +1 O# and Cl- has a -1 O# how do I balance that. And is what Ive done so far correct? Cr(OH)4- --> CrO42- Im confused on how to balance the oxygen and hydrogens ...
November 25, 2011 by Monique

Chemistry
Suppose that 30.0 mL of 0.20 M C6H5COOH(aq) is titrated with 0.30 M KOH(aq). (a) What is the initial pH of the 0.20 M C6H5COOH(aq)? (b) What is the pH after the addition of 15.0 mL of 0.30 M KOH(aq)? (c) What volume of 0.30 M KOH(aq) is required to reach halfway to the ...
November 3, 2010 by Alania

Chem 1A
A 15.00 g sample of an ionic compound NaA, where A- is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 700.0 mL of HCl was added, the pH was 5.00. The experimenter found that 1.40 L of 0.100 M ...
March 15, 2012 by Ashley

Chemistry UGH
Help please! I can't solve any of these, would someone be as kind as to show me the answers? How many moles of NaHCO3 are in a 125.0 g sample of the compound? 3. How many moles are in 6.73 x 1024 water molecules? 4-5. AgBr, a chemical used in photography can be made with this ...
May 28, 2009 by Daniel

Chemistry
Suppose you had an unknown solution that contained either dissolved NaCL, or NaNO3. You added AgNO3 to the unknown solution and observed that no solid forms. What can be concluded about the unknown solution? (use the solubility rules
April 25, 2011 by Lou

Chemistry
Suppose you had an unknown solution that contained either dissolved NaCL, or NaNO3. You added AgNO3 to the unknown solution and observed that no solid forms. What can be concluded about the unknown solution? (use the solubility rules
April 25, 2011 by Lou

AP Chemistry
In the titration of 50.0 mL of 1.0 M CH3NH2 (kb=4.4 x 10^-4), with 0.50 M HCl, calculate the pH a) after 50.0 mL of 0.50 M has been added b) at the stoichiometric point.
March 29, 2009 by some kid

Chemistry
Suppose that 50.0 mL of 0.25 M CH3NH2(aq) is titrated with 0.35 M HCl(aq). (a) What is the initial pH of the 0.25 M CH3NH2(aq)? (b) What is the pH after the addition of 15.0 mL of 0.35 M HCl(aq)? (c) What volume of 0.35 M HCl(aq) is required to reach halfway to the ...
November 3, 2010 by Dana

Bio (please help me, important)
In my bio lab we are creating serial disk dilutions (100mg, 300mg, 500mg) from a plant extraction sample. Wood sample #1 (7mL of hexane) Hexane 0.6651g so .6651g of the plant was dissolved in 7mL of hexane. Then I did dilution calculations so 0.6551g/7 mL = 0.095g/ml so I ...
January 3, 2007 by Ali

chemistry
mix 120ml of 0.320M silver nitrate with 40ml of 0.320M potasium chromate. What mass of silver chromate is produced? this is what i have so far 2AgNO3 + K2CrO4 --> Ag2CrO4 + 2KNO3 molar mass of 2agno3 = 277.81 molar mass of k2cro4 = 194.2 molar mass of ag2cro4 = 331.8 ...
January 29, 2010 by Krissy

Chemistry
Why would NAOH solution need to be added when preparing the K2CrO4 stock solution?
September 14, 2009 by Rose

Chem 111
Why would NaOH solution need to be added when preparing the K2CrO4 stock solution
January 31, 2013 by Bandar

biochemistry
Calculate the pH change of 10mL of HCl added to 1M phosphate buffer in 1L with initil pH of 7.2?
September 28, 2010 by Lina

science
the hydrogen ion concentration in a mixture of 10ml 0.1 M H2SO4 AND 10ml 0.1M KOH solution in water is?
August 22, 2014 by madhu

Chem
Help! I'm not suppose to react Iron Chloride with Silver Nitrate in order to get Iron nitrate. If i'm suppose to keep one of the above ingredients and obtain a pure dry sample, what should i do? I don't know the question. Why are you not supposed to react the two? and which ...
September 8, 2006 by kelly

chemistry
AgNO3 was dissolved in water to make 10mL of solution. Then 3.0mL of that solution was used to make a new solution with a total volume of 1.000L. What was the concentration of the silver ion in the final solution?
October 5, 2009 by Anonymous

chemistry
A chemist performed an experiment in which silver nitrate was used to precipitate all of the chromate ion as silver chromate, Ag2CrO4 from 200 mL of a solution of potassium chromate, K2CrO4. This process required 120 mL of 0.200 M AgNO3. Write the balanced equation that ...
October 10, 2011 by stephanie

Chemistry
Why is it desirable in the method of back-titration to have a considerable amount(more than 10mL) of acid added in excess?
February 27, 2011 by E

chemistry
For which of the following mixtures will Ag2SO4(s) (Ksp=1.20E^-5)precipitate? More than one answer can be selected. a.) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) b.) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq) c.) 150.0 mL of 0.10 M Na2SO4(...
November 6, 2012 by chem question

Chemistry
50.0mL of 1.04moles HA is added to 50.0mL if 0.90moles NH4OH.With a 1:1 stoichiometric ratio. What is the limiting reactant in moles of this reaction.
October 20, 2013 by Morgan

Science
Based on the following information: A series of chemicals were added to some AgNO3(aq). NaCl(aq) was added first to the silver nitrate solution with the end result shown below in test tube 1, NH3(aq) was then added with the end result shown in test tube 2, and HNO3(aq) was ...
December 2, 2012 by Spoa

AP Chemistry
In the titration of 77.5 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 10-4), with 0.38 M HCl, calculate the pH under the following conditions. (a) after 50.0 mL of 0.38 M HCl has been added (b) at the stoichiometric point
February 7, 2012 by Bill

Cemistry
A solution is 36% silver nitrate (AgNO3) by mass. The density of this solution is 1.44 g/mL. The formula weight of AgNO3 is 170 g/mol. Calculate the molality of AgNO3 in this solution.
June 9, 2010 by Swagato

Chemistry
if you have 100mL of 0.1M acetic acid (ka = 1.8x10(-5)what is the pH after 10mL NaOH is added? I came up with an answer of 2.895, but i'm not sure if its right.
October 26, 2011 by Kevin

CHEMISTRY
Suppose that 30.0 mL of 0.20 M C6H5COO(aq) is titrated with 0.30 M KOH(aq). a) What is the initial pH of the 0.20 M C6H5COOH(aq)? b) What is the pH after the addition of 15.0 mL of 0.30 M KOH(aq)? c) What volume of 0.30 M KOH(aq) is required to reach halfway to the ...
September 29, 2011 by Sarah

chemistry
3.50 mol Al(NO3)3 reacts with 5.00 mols K2CrO4, the total number of moles of Al2(CrO4)3 and KNO3 would be? Here is the equation if it's needed. 2 Al(NO3)3(aq) + 3 K2CrO4(aq) → Al2(CrO4)3(s) + 6 KNO3(aq)
December 12, 2012 by Michelle

Chemistry
what volume of water must be added to 10ml og 6.0M NaOH to make a solution that is .30 M in NaOH How do I solve for this
October 25, 2007 by Lauren

chemistry
A 30.00mL sample of a clear saturated solution of PbI2 requires 14.7mL of a certain AgNO3 for its titration. I^-(saturated PbI2)+Ag^+(from AgNO3)--> AgI(s) What is the molarity of this AgNO3? I'm not really sure where to start.
March 16, 2012 by brad

Chemistry
Suppose you wanted to find out how many milliliters of 1.0 M AgNO3 are needed to provide 169.88 g of pure AgNO3. a. What is step 1 in solving the problem? b. What is the molar mass of AgNO3? c. How many milliliters of solution are needed?
April 22, 2013 by Somer

Physical chemistry 2
50 ml of 0.02M acetic acid is titrated with 0.1M NaOH.Calculate the pH of the solution when 10ml of NaOH is added
March 12, 2013 by Anonymous

chemistry
Silver nitrate (AgNO3) reacts with sodium chloride as indicated by the equation AgNO3 + NaCl ! AgCl + NaNO3 . How many grams of NaCl would be re- quired to react with 511 mL of 0.38 M AgNO3 solution? Answer in units of grams
September 19, 2012 by cheri

Chemistry
1) 800 mL of 0.025 M Pb(NO3)2 is mixed with 500 mL of 0.030 M K2CrO4. Calculate the grams of PbCrO4 that form. I am confused on how to do this I got the answer it should be 4.85 g PbCrO4, but I would want to know how to get that. And also Limiting reactant is K2CrO4, but I don...
April 4, 2012 by Akbar

chemistry
Using your 0.0100M oxalate solution and only the equipment and supplies listed below, describe how to prepare a 0.00025M solution of oxalate. Note, you are not allowed to add volumes with pipettes. (example, if you want 20mLs, you can not use a 10mL + 10mL addition as this ...
June 17, 2013 by Annie

Chemistry
Using your 0.0100M oxalate solution and only the equipment and supplies listed below, describe how to prepare a 0.00025M solution of oxalate. Note, you are not allowed to add volumes with pipettes. (example, if you want 20mLs, you can not use a 10mL + 10mL addition as this ...
June 17, 2013 by Jessica

Chemistry
Question: you have a clear, colorless aqueous sample in a beaker that contains either CO2^-2(aq) or C^-1(aq) or a mixture of both ions. the following aqueous reagents are available: NaCl, HNO3, and AgNO3. describe a procedure that will allow the determination of which of the ...
May 12, 2009 by Anonymous

Chemistry
Silver nitrate (AgNO3) reacts with sodium chloride as indicated by the equation AgNO3 + NaCl ! AgCl + NaNO3 . Howmany grams of NaCl would be required to react with 518 mL of 0.543 M AgNO3 solution? Answer in units of grams
October 4, 2011 by Broy

chemistry
A stock solution's hypochlorite activity was determined as follows: . - 2.00g of liquid sodium hypochlorite (NaOCl) was weighed into a flask and diluted with 50mL deionized water.10mL of 10% sulfuric acid and 10mL of 10% potasssium iodide were added, followed by titration with...
August 4, 2010 by angela

chem
If 60.0 mL of 0.150 M CaCl2 is added to 50.0 mL of 0.100 M AgNO3, what is the mass in grams of AgCl precipitate?
March 2, 2009 by ash

Chemistry
CO(h20)6 2+ + 4Cl- <=> CoCl4 2- + 6H20 What would AgNO3 do when added to this? What is the equilibrium expression?
March 9, 2010 by Kharris

Chemistry
CO(h20)6 2+ + 4Cl- <=> CoCl4 2- + 6H20 What would AgNO3 do when added to this? What is the equilibrium expression?
March 9, 2010 by Kharris

chem
5 drops of AgNO3 must be added to 1 L of a water sample: 46.1 mg SO42-/L and 30.6 mg Cl -/L. What will be the precipitate that forms?
April 22, 2010 by Tommy

chemistry
If 30.0 mL of 0.150 M CaC12 is added to 15.0 mL of 0.100 M AgNO3, what is the mass in grams of AgC1 precipitate?
September 29, 2010 by Michael

chemistry
if 30ml of .150 M CaCl2 is added to 22.5ml of .1 M AgNO3, what is the mass of the AgCl precipitate?
October 11, 2010 by jenna

Chemistry
Suppose that 30.0 mL of 0.20 M C6H5COOH(aq) is titrated with 0.30 M KOH(aq). Refer to table 1 and table 2. (a) What is the initial pH of the 0.20 M C6H5COOH(aq)? Using ICE i found to be 2.46 The rest I do not know how to set up or solve... (b) What is the pH after the addition...
March 12, 2010 by Val

Chemistry
an acid base titration is conducted in which 20 ml of LiOH is added to 10ml of .200M HBr to reach the equivilance point. what is the molarity of the LiOH solution?
April 12, 2010 by Elf

Chemistry
I recently did an experiment on Aldol Condensation, by reacting Benzaldehyde with Acetone to form Dibenzalacetone. The proposed stoichiometric ratio of Benzaldehyde:Acetone is 2:1. What would be the implications if either of the reactants is in excess?
February 12, 2010 by Alan

Chemistry
Refer to the net ionic equation below to answer the following questions: Co(H2O)6^+2 + 4Cl- <==> CoCl^-2 + 6H2O 1. In what direction was the equilibrium shifted by: a. Addition of HCl b. Addition of water c. Addition of AgNO3 d. Increasing the temperature e. Decreasing ...
January 21, 2011 by Sharon

Chemistry
Why does equilibrium shift to the left when AgNO3 is added to the equation Co(H20)6 (aq) + 4Cl- (aq) <---> CoCl4 (aq) + 6H2o(l)?
April 8, 2012 by Nancy

Chemistry
What is the ionic equations for the following metals and aqueous substances? With the same equation what is being oxidize and what is being reduced? Zn + AgNO3 Zn + CuSO4 Zn + PbNO3 Mg + AgNO3 Mg + CuSO4 Mg + PbNO3 Cu + AgNO3
November 21, 2010 by Jose-Ann

Chemistry
IN my experiment, I was doing a qualitative analysis of Group I and II anions using a flowchart. IN the chart I added 5 drops of 0.1M AgNO3 and several drops of 3M HNO3 to 5 drops of solution and found that a precipitate was formed. Thus it was classified as a Group I anion. ...
April 12, 2009 by David

stoichiometry
When Ba(NO3)2 and K2CrO4 (sorry, i don't know how to do subscripts, but all the numbers should be subscripts!) react in aqueous solution, the yellow solid BaCrO4 is formed. Calculate the mass of BaCrO4 that forms when 3.50 x 10^(-3) mol of solid Ba(NO3)2 is dissolved in 265 mL...
June 5, 2008 by em

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