# When 20.0 mL of 0.100 M AgNO3 are mixed with 80.0 mL of 0.0100 M Na2CrO4, what is the chromate ion concentration (CrO4^2-)? Ksp for Ag2CrO4 = 9.0 x 10^-12. I think it's 1.0 x 10^-9. Am I right?

22,864 results
1. ## Chemistry

Which two solutions, when mixed together, will undergo a double replacement reaction and form a white, solid substance? 1. NaCl(aq) and LiNO3(aq) 2. KCl(aq) and AgNO3(aq) 3. KCl(aq) and LiCL(aq) 4. NaNO3(aq) and AgNO3(aq) I know the answers 2 but I have no

2. ## AP Chemistry

We add excess Na2CrO4 solution to 68.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.270 grams. What is the molarity of the AgNO3 solution? Answer in

3. ## College Chemistry

How many milliliters of 0.100 M HNO3 are needed to neutralize the following solutions? A. 45.0 mL of 0.667 M KOH B. 58.5 mL of 0.0100 M Al(OH)3

4. ## 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

5. ## Chemistry

Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) 2NOCl(g) Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10–4 2 0.0150 0.0100 8.5 x 10–5 3 0.0150 0.0400 3.4 x 10–4 a. 1.13 M –2s–1 b. 9.44 M

6. ## 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?

7. ## Chemistry

You have 75.0 mL of a 2.50 M solution of Na2CrO4 (aq). You also have 125 mL of a 2.15 M solution of AgNO3 (aq). Calculate the concentration of NO3 when the two solutions are added together.

8. ## Chemistry

What is(are) the precipitate(s) that form when K2SO4, BaCl2, and AgNO3 solutions are mixed?

9. ## Chemistry

How many milliliters of .100 M HNO3 are needed to neutralize 58.5 mL of .0100 Al(0H)3?

10. ## chemistry

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 „e 10¡V12] What is the concentration of the silver ion remaining in solution?

11. ## Chemistry

At what temperature will 0.0100 mole of argon gas have a volume of 275 mL at 100.0 kPa?

12. ## chemistry

We are doing a lab that requires finding the molarity of an unknown AgNO3 solution after reacting NaCl + AgNO3 --> NaNO3 and AgCl and collecting/massing the precipitate. We will be using 10.00 mL of an NaCl solution and 10.00 mL of the AgNO3 solution. We

13. ## calculus

For which of the following mixtures will Ag2SO4(s) precipitate? 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq) 150.0 mL

14. ## AP CHEM

Silver nitrate (AgNO3) reacts with sodium chloride as indicated by the equation AgNO3 + NaCl → AgCl + NaNO3 . How many grams of NaCl would be required to react with 132 mL of 0.719 M AgNO3 solution? Answer in units of grams.

15. ## CHEMISTRY

1. You have 88.8 mL of 2.50 M solution of Na2CrO4 (aq). You have 125 mL of a 2.50 M solution of AgNO3 (aq). Calculate the concetration of Na+ when the two solutions are added together. 2. You have 75.0 mL of 2.50 M solution of Na2CrO4 (aq). You have 125 mL

16. ## Chemistry

What is the concentration of NO3- ions when equal volumes of 0.1M AgNO3 and 0.1M NaCl are mixed together?

17. ## chemistry

Which of the following experimental conditions describe a reaction which is kinetically controlled? These conditions do not describe kinetic control. ΔG = -100 kJ/molrxn; there is no observable reaction when reactants are mixed. ΔG = +100 kJ/molrxn;

18. ## Chemistry

At what tempature will .0100 moles of argon gas have a volume of 275mL at 100 kPa? please this is due tommorrow really need som help

19. ## Chemistry

what mass of AgBr is formed when a solution containing 3.45 g of KBr is mixed with a solution containing 7.28 g AgNO3?

20. ## biology

100 ml of agno3 at 0.1g/ml

21. ## Chemistry

What is the Qsp when 59.0 mL of 2.00 multiplied by 10-4 M AgNO3 are mixed with 70.0 mL of 1.00multiplied by10-4 M Na2CrO4? Assume the volumes are additive. Ksp = 1.1 multiplied by 10-12.

22. ## Chemistry

Identify the solid product that forms when the following aqueous solutions are mixed Na2CrO4+BaCl2= AnNO3+NH4Cl= I assume in the second that should be silver nitrate. Barium dichromate and silver chloride are not soluble, are they?

23. ## math

17. 0.0101 , 0.0100, 0.0110,0.0011 Using the numbers above, which of the following sequences lists the numbers from least to greatest? A. 0.0011, 0.0100, 0.0101 , 0.0110 B. 0.0110, 0.0101 , 0.0100, 0.0011 C. 0.0011 , 0.0101, 0.0100, 0.0110 D. 0.0110,

24. ## Science

A mixture is prepared by adding 100 ml of 0.10M Na2CrO4 to 100.ml of ).10 N AgNO3. A precipitate forms in this mixture. The precipitate is separated from the mixture by filtration. Question: What quantity of solid product is produced?

25. ## Chemistry

Consider the following reaction AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq) DH = -66 kJ Suppose that 100.0 mL of 0.100M AgNO3 is added to 200.0 mL of 0.100 M NaCl in a coffee cup calorimeter. Assuming that the initial temperature of the solution is

26. ## Chemistry

For the reaction 4A (g)+3B (g)=C(g) the following data were obtained at constant temperature: Experiment- 1. Initial (A) (mole/L) 0.0500, 01000, 01000 , 0.0500 2. Initial (B) (mole/L) 0.0500, 0.0500, 0.1000, 0.0500 3. Initial (C)(mole/L) 0.0100, 0.0100,

27. ## 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

28. ## chemistry

Thimerosal is an organic compound (gram molecular mass = 404.8 g/mol) used to inhibit bacterial growth. A .100%solution of thimerosal is sometimes used as an antiseptic. Assume that this solution has a density of 1.00 g/mL. A. how many grams of thimerosal

29. ## Chemistry

Calculate the value of the reaction quotient, Q, of silver iodate (AgIO3) when 10.0 mL of 0.011 M AgNO3 is mixed with 10.0 mL of 0.02 M NaIO3. Can you please explain the process?

30. ## 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.

31. ## Chemistry

Quantitative anaylsis of cl- ion is often performed by a titration with silver nitrate, using sodium chromate as an indicator. As standardized AgNo3 is addded, both white AgCl and red Ag2CrO4 precipitate, but so long as some cl- remains, the Ag2CrO4

32. ## Chemistry

When 20.0 mL of 0.100 M AgNO3 are mixed with 80.0 mL of 0.0100 M Na2CrO4, what is the chromate ion concentration (CrO4^2-)? Ksp for Ag2CrO4 = 9.0 x 10^-12. I think it's 1.0 x 10^-9. Am I right?

33. ## chemistry

You have 95.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.50 M solution of AgNO3(aq). Calculate the concentration of Na+ after the two solutions are mixed together. 1.08 M 0.475 M 5.00 M 0.00 M 2.16 M

34. ## CHEMISTRY

When 50.0 cm3 of 0.100 mol dm-3 AgNO3 is mixed with 50.0 cm3 of 0.0500 dm-3 HCl in a polystyrene cup, the temperature increases from 20.00°C to 20.35°C. Assume that the specific heat capacity of the solution is the same as that of water, and that the

35. ## Chem

In a coffee cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed to yield the following reaction: Ag+ (aq) + Cl- (aq) -----------------> AgCl (s) The two solutions were initially at 22.60 °C, and the final temperature is 23.40

36. ## chemistry

Can Anyone Help Me With This Solubility Problem? An aqueous solution of 1.90 M AgNO3 is slowly added from a buret to an aqueous solution of 0.0100 M Cl- and 0.250 M I-. b) When the second ion begins to precipitate, what is the remaining concentration of

37. ## math

17. 0.0101 , 0.0100, 0.0110,0.0011 Using the numbers above, which of the following sequences lists the numbers from least to greatest? A. 0.0011, 0.0100, 0.0101 , 0.0110 B. 0.0110, 0.0101 , 0.0100, 0.0011 C. 0.0011 , 0.0101, 0.0100, 0.0110 D. 0.0110,

38. ## Chemistry

Calculate the Ksp of a saturated solution of Mg(OH)2 upon titration with 0.0100 HCl in the presence of phenolphthalein indicator utilizing the data below. mL saturated Mg(OH)2 titrated - 1382 mL of 0.0100 M HCl to endpoint - 38.7 Please help me and show

39. ## Chemistry

Given the rate equation... RATE = ([ Na2S2O3]/time) = k [I-]a [BrO3-]b [HCl]c 1A) You mix together in the proper manner the following: 10.0 mL of .0100 M Potassium Iodide 10.0 mL of .00100 M Sodium thiosulfate 10.0 mL of water 10.0 mL of .0400 M Potassium

40. ## chemistry

RATE = ([ Na2S2O3]/time) = k [I-]a [BrO3-]b [HCl]c 1A) You mix together in the proper manner the following: 10.0 mL of .0100 M Potassium Iodide 10.0 mL of .00100 M Sodium thiosulfate 10.0 mL of water 10.0 mL of .0400 M Potassium Bromate 10.0 mL of .100 M

41. ## 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.

42. ## chemistry

A stock solution of 0.0100 M KMnO4 is diluted by taking 15.5 mL of it and diluting it to 100.0 mL. From this diluted solution, 5.00 mL is taken out and diluted to 100.0 mL. What is the concentration of the solution obtained in the end

43. ## Chemistry

Will AgCl precipitate out when equal amounts of 4.0 × 10-5M AgNO3 and 1.0 × 10-5M NaCl are mixed? (Ksp for AgCl = 1.8 × 10-10)

44. ## Chemistry

Solution of 50g AgNO3 is mixed with 50g NaCl. a) What mass of AgCl will you get? b) which substance is in redundancy?

45. ## Chemistry

Hi! I kind of need help to get started with these four problems. There are more problems like the ones below. It would be great if I had an example of each of the four problems. Thanks! FeSO4(aq)+ KCL(aq) (for problem 1 and 2) 1)When the following

46. ## Chemistry

A 0.60 L portion of a 1.2 M AgNO3 solution is mixed with a 0.3 L potion of a 1.2 M Na2CrO4 solution in an constant pressure calorimeter. Upon mixing, the solid Ag2CrO4 is formed and the heart released is 48.2 kJ. The specific heat of the solution is 4.18

47. ## chemistry 101

We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.590 grams. What is the molarity of the AgNO3 solution? Answer in

48. ## 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!

49. ## Chemistry

please show me step by step how to do this so i can figure out the rest We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to

50. ## chemistry

A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nintric acid,500. mL of 0.0100 M calcium hydroxide, and 200.0 mL

51. ## Chemistry

A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nintric acid,500. mL of 0.0100 M calcium hydroxide, and 200.0 mL

52. ## chemistry

A student mixes 4 reagents together thinking that the solution will neutralize each other . The solutions are mixed together are 50 ml of 0.100 M .hydrochloric acid 100 ml of 0.200 M of nitric acid 500 ml of 0.0100 M calcium hydroxide and 200 ml of 0.100 M

53. ## Science

You have 75.0 mL of a 2.50 M solution of Na2CrO4 (aq). You also have 125 mL of a 2.15 M solution of AgNO3 (aq). Calculate the concentration of NO3 when the two solutions are added together.

54. ## chemistry

what mass of AgNO3(MW 169.87) is required to make 25 mL of 0.100 M AgNO3?

55. ## AP Chemistry

in a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M of HCl are mixed to yield the following reaction: Ag+ (aq) + Cl- (aq) >> AgCl (s) the two solutions were initially at 22.60 degree celsius, and the final temperature is 23.40

56. ## chemistry

To a 100.0 mL solution containing 0.0100 M Ba(NO3)2 and 0.0100 M Pb(NO3)2 was added 101.0 mL of 0.0100 M H2SO4 to provide a slight excess of SO42- relative to Ba2+ in the resulting solution. Assuming that: i) H+ does not bind to SO42- ii) ionic strength

57. ## chemistry

mL of 0.0100 M NaOH are added to 25.0 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?

58. ## chemistry

Determine the percentage composition of each of the following compounds a) NaCl b) AgNO3 c) Mg(OH)2 for NaCl i got na=23/135=0.17 x 100= 17% Cl=35/135=0.26 x 100=26% for AgNO3 i got 108/42 which im sure was wrong and i didn't get how to complete the

59. ## Chemistry!

0.0100 Ba(OH)2 is dissolved in water to give 500.0 mL of solution calculate OH- concentration would it be the molarity of Ba(OH)2 (0.0100 / 0.500) multiplied by two because there is twice as much OH??

60. ## Math

Write as a fraction or mixed number: 1) 0.85 2) 3.6 3) 0.888... We read 0.85 as eighty-five hundredths. Expressed as a fraction it's 85/100. Please tell us what you think the other two numbers are expressed as a fraction or mixed number. We'll be glad to

61. ## chemistry

caculate the mass of agcl precipitated when 0.1g of nacl and 0.1g of agno3 are mixed in solution

62. ## chmeistry

50 ml of 0.1 M NaCl is mixed with 50 ml of 0.2 M AgNO3 predict whethera ppt of AgCl is formed or not

63. ## chemistry

At some other temperature, a solid sample of Ca(OH)2 is shaken with 0.0100 M CaCl2. Once equilibrated, some solid Ca(OH)2 remains undissolved. The solution is filtered and a 20.00 mL sample requires 38.80 mL of 0.0100 M HCl to neutralize it. Calculate the

64. ## Chemistry

Given the rate equation... RATE = ([ Na2S2O3]/time) = k [I-]a [BrO3-]b [HCl]c 1A) You mix together in the proper manner the following: 10.0 mL of .0100 M Potassium Iodide 10.0 mL of .00100 M Sodium thiosulfate 10.0 mL of water 10.0 mL of .0400 M Potassium

65. ## chemistry

Can Anyone Help Me With This Solubility Problem? An aqueous solution of 1.90 M AgNO3 is slowly added from a buret to an aqueous solution of 0.0100 M Cl- and 0.250 M I-. a) Which ion, Cl- or I-, is the first to precipitate? b) When the second ion begins to

66. ## Chem

A 50 ml sample of 0.025M AgNo3 is mixed with 15 ml of 0.04 M CrCl3. How many grams of AgCl will precipitate? Please show steps

67. ## Chemistry/pH- Weak Acid

in response to Chemistry/pH- Weak Acid. but the rule of 5%? 0,0100/(1.00x10^-4) =100% The aproximation you do is not valid...or? Ka= (1,0*10^(-4))^2/(x-1*10^(-4) )=1,00*10^(-6)....I got c=0,0101M :-(

68. ## Chemistry

A quantity of 100 mL of .5M of HCl (aq) is mixed with 100 mL of .5M of NaOH (aq) in a constant pressure calorimeter. The initial temperature of the solutions is 22.30 C and the final temperature of the mixed solution is 25.00 C. What is "q" for solution

69. ## Chemistry

Equal volumes of 0.240 M AgNO3 and 0.140 M ZnCl2 solution are mixed. Calculate the quilibrium concentrations of Ag+, and Zn2+.

70. ## Chemistry 101

This is a different question then asked before,I had lab where I mixed 1.365 NaCL + AgNO3-->2.6242 AgCl. The 2 questions that I need help finding the answers to are: How much salt should be used to cause all of the silver nitrate to react? How much silver

71. ## Science (chemistry) help please

The following data was obtained from titrating a solution containing 25 mL of 0.0100 M MgCl2 solution, 1 mL of NH3OH buffer, and 10 drops of Calmagite with EDTA. Calculate the concentration of EDTA. Report the answer with three sig figs. I don't know what

72. ## Math check

write the decimal as a fraction or a mixed number in simplest form 2.67 2.67/1× 100/100 = 267/100 267/100 = 2 67/100?

73. ## 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

74. ## AP CHEM

Silver nitrate (AgNO3) reacts with sodium chloride as indicated by the equation AgNO3 + NaCl → AgCl + NaNO3 . How many grams of NaCl would be required to react with 132 mL of 0.719 M AgNO3 solution? Answer in units of grams.

75. ## 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

76. ## Chemistry 101

I had a snag from a question I asked yesterday, here is the thread. (My snag being the final post) I am trying to find the theoretical yield for this lab I am working on. The steps to finidng it would be great. In my lab I took 40mls of H2O + 4g of AgNO3+

77. ## Chemistry

2. Does a precipitate of silver chloride form when 200.0 mL of 1.0 x 10-4 M AgNO3 (aq) and 900.0 mL of 1.0 x 10-6 M KCl (aq) are mixed at 25oC?[ Ksp AgCl @ 25oC = 1.6 x 10-10]

78. ## Chemistry

predict if precipitation will occur when 36ml of 0.0039M Na2CrO4 is mixed with 18ml of 0.00033M AgNO3. M.W of Ag2CrO4 :331.73g/mol Kspof ag2cro4 1.1x10^-12

79. ## chem 101

We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.590 grams. What is the molarity of the AgNO3 solution? Answer in

80. ## chemistry

We add excess Na2CrO4 solution to 27.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.420 grams. What is the molarity of the AgNO3 solution? Answer in

81. ## chemistry

What mass of Na2CrO4 is required to precipitate all of the silver ions from 71.0 mL of a 0.101 M solution of AgNO3?

82. ## AP Chemistry

What mass of Na2CrO4 is required to precipitate all the silver ions from 96.0 mL of a 0.650 M solution of AgNO3?

83. ## AP Chemistry

Please show me how to do this step by step I would appreciate it We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.520

84. ## chemistry

a student mixes 4 reagents together thinking that the solution will neutralize each other . The solution is mixed together are 50 ml of 0.100 M of HCL and 100 ml of 0,200 M of nitric acid 500 ml of 0.0100 M ca hydroxide and 200 ml of 0.100 M rubidium

Will Na2CrO4 react exactly the same as Na2CrO7 when mixed with Pb(NO3)2

86. ## Chemistry

you have75.0ml of 2.5 M Solution of Na2CrO4(aq). You also have 125ml of a 1.74M solution of AgNO3(aq)Calculate the concentration of NO3 when the two solutions are added together

87. ## CHEMISTRY

In a coffee cup calorimeter 70.0 mL of 0.100 M AgNO3 and 70.0 mL of 0.100 M HCl are mixed to yield the following reaction. Ag+(aq) + Cl ‾(aq) → AgCl(s) If the two solutions are initially at 22.60°C, and if the final temperature is 23.39°C, calculate

88. ## chemistry

Calculate the concentrations of all ions after 50.0 mL of a 0.100 M AgNO3 solution is mixed with 100.0 mL of a 1.00 M Na2SO4 solution.For Ag2SO4 Ksp = 1.2 x 10-5 Do I first do MiVi=MfVf and then using the two concentrations I use ksp value? I'm just so

89. ## Chemistry

How many grams of AgNO3 will precipitate when 150 mL of 0.5 M AgNo3 adds to 100 ml 0.4 M KCrO4? Please answer immediately.

90. ## AP Chemistry

in a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M of HCl are mixed to yield the following reaction: Ag+ (aq) + Cl- (aq) >> AgCl (s) the two solutions were initially at 22.60 degree celsius, and the final temperature is 23.40

91. ## chemistry

8 mL of 0.0100 M HCl are added to 22 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?

92. ## Chemistry

11 mL of 0.0100 M HCl are added to 25 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?

93. ## chemistry

Common ion effect;At some other temperature, a solid sample of Ca(OH)2 is shaken with 0.0100? Common ion effect;At some other temperature, a solid sample of Ca(OH)2 is shaken with 0.0100 M CaCl2. Once equ? At some other temperature, a solid sample of

94. ## Chemistry

1. A graduate measured out a 100. mL hard water sample and titrated it with 37.6 mL of 0.0100 M EDTA solution for a total hardness endpoint, and 29.3 mL of 0.0100 M EDTA solution for a calcium endpoint. Calculate the molarity with respect to magnesium and

95. ## Chemistry

When 5.4 g of NaCl and 3.6 g of AgNO3 are dissolved in water and mixed, what ions remain in the solution and how many moles of each will be there?

96. ## chemistry

Find the Qsp when 5 mL of 0.17 M K2 CO3 (aq) and 1 L of 0.013 M AgNO3(aq) are mixed together. The solubility product of Ag2CO3 is 6.2 × 10−12

97. ## chemistry

How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 5.05 help please :(

98. ## St. Michael

25ml of NaCl was mixed with 10ml of AgNO3. A precipitate was made. What is the theoretical yield? What is the limiting and excess reagent?

99. ## 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

100. ## chem101

If a solution contains 0.0100 mole of HCl in 10.0 mL aqueous solution. a.) What is its molarity? My answer is 1M (0.0100 mole/10.0 mL * 1000 mL/1L = 1M) b.) What is H^+ ion concentration for this solution? c.) What is the expected pH for this solution? pls