# Calculate mole solute in solution? I added an amount of an unknown sample to a solution. I found that the molality of the solution is 0.085m and there is 0.0156kg of solvent. Calculate the moles of solute present in solution?

79,209 results
1. ## chemistry

CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be

2. ## Chemistry

Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. Solution A: 10.0 mL 3.0e-4M bromescol green

3. ## Chemistry

An aqueous solution is 8.50% ammonium chloride, NH4Cl, by mass. The density of the solution is 1.024g/mL. Calculate the molality, mole fraction, and molarity of NH4Cl in the solution. I know the formulas needed but I'm not sure where to start. M = moles

4. ## chem

Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving .400 moles of MgCl2 in 850.0g of water. mole fraction =amount solute(in mols) /total amount of solute and solvent (in mols) so wouldn't it be .400/ .400+ 47.2 which is

5. ## Analytical chemistry

A 25.0-mL solution of 0.0660 M EDTA was added to a 33.0-mL sample containing an unknown concentration of V3 . All V3 present formed a complex, leaving excess EDTA in solution. This solution was back-titrated with a 0.0450 M Ga3 solution until all the EDTA

6. ## chemistry

A 2.500×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3mL . The density of

7. ## AP Chemistry

A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with pure water, the pH does

8. ## chem

A solution is made by dissolving 27.8 g of nicotine (Molar Mass = 160 g/mol) in 145 g of cyclohexane (C6H12) to form 142 mL of solution. Calculate the mole fraction of the solute and the molarity, respectively, of this solution.

9. ## Chemistry

A solution is created by dissolving 13.0 grams of ammonium chloride in enough water to make 265 mL of solution. How many moles of ammonium chloride are present in the resulting solution? When thinking about the amount of solute present in a solution,

10. ## Chemistry

An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of NaCl of the same concentration. Which of the following substances could the unknown be: KOH,NH3,HNO3,

11. ## Chemistry

8 g of sulphur is burnt to form SO2 which is oxidized by Cl2 water The solution is treated with BaCl2 solution The amount of BaSO4 precipitated is A/ I mole B/ 0.5 mole C/ 0.24 mole D/. 0.25 mole Which option is correct??

12. ## Chemistry

The freezing point of a cyclohexane sample is 6.20*C. A soltuion is prepared by dissolving 0.4660g of an unknown solute in 36.0g cyclohexane. The freezing point of the solution if 4.11*C. Calculate the molar mass of the unknown solute. Kf for cyclohexane

13. ## Chemistry lab

A 1.340gram sample of an unknown acid, H3A, was placed in a 250.0 mL volumetric flask and diluted to volume with water. A 45.35 mL sample of this acid solution was titrated with 37.77 mL of a 0.1006M NaOH solution. A) Using one set - up dimensional

14. ## Chemistry

Calculate mole solute in solution? I added an amount of an unknown sample to a solution. I found that the molality of the solution is 0.085m and there is 0.0156kg of solvent. Calculate the moles of solute present in solution? Thanks!

15. ## chemistry

A 1.857 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.540 grams of KI and 50.00 mL of a 0.00912 M KIO3 solution. The excess I3– was

16. ## AP Chemistry

CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be

17. ## Chemistry

What does it mean to say that a solution is saturated with a solute? (Select all that apply.) a) A solute that is at equilibrium with undissolved solvent. b) A solvent that is at equilibrium with solute. c) A solution contains the maximum amount of solvent

18. ## Chemistry

Cyclohexane has a freezing point of 6.6 degree Celsius and a K(f) of 20.0 degree Celsius/m. 1.50g of an unknown solute is dissolved wth 18.0g of cyclohexane. The freezing point of the solution was 1.3 degree Celsius Using this iInformation assuming the

19. ## AP Chemistry

An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M I

20. ## AP Chemistry

An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

21. ## Chemistry

A 29.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 24.63 mL of NaOH solution is added? What is the concentration of the unknown H3PO4 solution? The neutralization reaction is

22. ## Chemistry

A water solution containing an unknown quantity of an unknown nonelectrolyte solute has a freezing point of -0.21 Celsius. What is the molality of the solution? Kf=-1.86C/m

23. ## Chemistry

Calculate mole solute in solution? I added 0.2968g of an unknown to a solution. I found that the molality of the solution is 0.085m and there is 0.0156kg of solvent. Calculate the moles of solute present in solution? Thanks!

24. ## chemistry

I need help on these questions. They all seem pretty similar i think? i don't know what formula i am suppose to use. And what does nonvolatile mean? is that like a clue or something? 1) 2.6 g of the nonvolatile solute sucrose (C12H22O11) is added to 465 g

25. ## chem

(5) In this experiment MnO4-is reduced to Mn 2+ by the unknown. What is the equivalent weight of MnO4- for this experiment? 52.68 (6) How many equivalents of electrons were transferred from the unknown solution? (7) What is the Normality of the 1.00 mL of

26. ## Chemistry

A 2.304 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.500 grams of KI and 50.00 mL of a 0.00912 M KIO3 solution. The excess I3– was

a) To make an acid solution, 6.8 x 10-3 mole of a strong acid (6.8 x 10-3 mole H3O+) is dissolved in water to give a 550 mL solution. What is the pH and [OH-] of the solution? b) 150 mL of water is added to 50 mL of the solution produced in question 3.

28. ## Chemistry

A is a solution of trioxonitrate (V) acid. HNO of unknown concentration B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution 25cm3 portion solution B required an average of 24.00cm3 of solution A for neutralization. Using 2 drop

29. ## chemistry

Student A prepared a solution by dissolving 8.00 g potassium perchlorate in 72.0 g H2O. Given that the density of potassium perchlorate solution is 2.524 g/mL at 25 degree C . (a) Calculate the % by mass of solute of the potassium perchlorate solution. (b)

30. ## chemistry

A 27.00 mL sample of an unknown H3PO4 solution is titrated with a 0.110 M NaOH solution. The equivalence point is reached when 25.78 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is:

31. ## 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

32. ## CHEMISTRY.

Lowering of vapor pressure is directly proportional to: a) Temperature b) Mole fraction of Solute c) Mole fraction of Solvent d) Amount of solution

33. ## chemistry

Copper can be determined gravimetrically by precipitation as copper(I)thiocyanate, CuSCN. A wrought aluminum-copper sample(4.5167 g) was dissolved in a minimum amount of concentrated HCl followd by the additon of 25 ml of sulfurous acid to reduced the

34. ## Chemistry

a 25.0 mL sample of .050 M solution of aqueous trimethylamine is titrated with a .063 M solution of HCl. calculate pH the solution after 10.0 mL, 20.0 mL, 30.0 mL of acid have been added. pKb of (CH3)_3_N= 4.19 at 25 degrees C

35. ## Chemistry

I have a test on monday and I NEED to ace it in order to raise my grade > . < ldsfkjaslkf right now, acids and bases are killing me can somebody help me with these problems? A buffer solution is prepared by mixing the weak base ammonia (Kb=1.77x10^-5) with

36. ## AP Chemistry

A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of

37. ## Chemistry

A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of

38. ## Chemistry

I have to match the items to the statements below, and I'm stuck! A Dilute B Unsaturated C Saturated D Supersaturated 1. Sodium acetate solution after the excess solute fell out of solution. 2. There is visible solute on the bottom of the container. 3. The

39. ## Chemistry

An unknown amount of water is mixed with 310 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 58.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

40. ## Chemistry

An unknown amount of water is mixed with 310 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 58.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

41. ## Chemistry

An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 51.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

42. ## Chemistry URGENT

I have to match the items to the statements below, and I'm stuck! My answers are in parentheses, but I know that some of them are wrong. Please help if you know how...I would GREATLY appreciate it! A Dilute B Unsaturated C Saturated D Supersaturated 1.

43. ## CHEMISTRY

n unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52 . 5 mL of 6 M HCl. Calculate the concentration of the di- luted NaOH solution. Answer in units of

44. ## chemistry

You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured

45. ## Science, Chemistry

A 25.0 mL sample of a 0.0600 M solution of aqueous trimethylamine is titrated with a 0.0750 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C. I already calculated pH

46. ## Chemistry

a) To make an acid solution, 6.8 x 10-3 mole of a strong acid (6.8 x 10-3 mole H3O+) is dissolved in water to give a 550 mL solution. What is the pH and [OH-] of the solution? b) 150 mL of water is added to 50 mL of the solution produced in question 3.

47. ## chemistry

You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured

48. ## Chem

I need to calcuted the molarity from this 12.5 g of ethylene glycol antifreeze dissolved in o.100kg of water. Density of solution is 1.0 g/mL I know molarity if mole of solute / L of solution. I am confused on how to find the L of solution. Do I add 12.5

49. ## chemistry

10.0 mL of a Cu2+ solution of unknown concentration was placed in a 250 mL Erlenmeyer flask. An excess of KI solution was added. Indicator was added and the solution was diluted with H2O to a total volume of 75 mL. The solution was titrated with 0.20 M

50. ## CHEM

Mass percent is one way to represent solution concentrations, though not the only one. A common measure of solution concentration is Molarity; moles of solute per liter of solution. Calculate the molarity of vinegar in each sample that you titrated and

51. ## chemistry

a. Find the amount of solute based on this information Volume = 500 ml Concentration of solution= 15% (w/w) Solute (molar mass) = H2SO4 is 98.0g/mol b. Find the molar mass Amount of solute= 117.0g Volume of solution= 2.00L concentration of a solution= 1.0M

52. ## chemistry

a. Find the amount of solute based on this information Volume = 500 ml Concentration of solution= 15% (w/w) Solute (molar mass) = H2SO4 is 98.0g/mol b. Find the molar mass Amount of solute= 117.0g Volume of solution= 2.00L concentration of a solution= 1.0M

53. ## chemistry

1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute is present in 1200g of

54. ## Chemistry

1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute is present in 1200g of

55. ## Chemistry

Calculate the amount of solute needed to make each of the solution: 225g of 10% (m/m) K2CO3 solution .50kg of a 18% (m/m) KOH solution

56. ## 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

57. ## 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

58. ## chemistry

Calculate the amount of solute needed to make each of the solution. 225g of a 10% (m/m) K2CO3 solution .50kg of a 18% (m/m) KOH solution please show work thanks

59. ## Chemistry

25g of a sample of ferrous sulphate was dissolved in water containing dilute h2s04 and the volume made up to one litre. 25ml of this solution required 20ml of N/10 kmn04 solution for complete oxidation. Calculate the percentage of f2s04 7h20 in the sample

60. ## Chemistry

When 2.50g of an unknown solute is dissolved in 40.0g of ethanol the solution boils at 79.4C. The normal boiling point of this substance is 78.4C and it has a kb of 1.22C/m. (a) What is the molality of this solution? (b) What is the molecular weight of the

I would appreciate very much If you guys could show me how to approach this problem. A solution is prepared by dissolving 10.8g of ammonium sulfate in enough water to make 100.0mL of stock solution. A 10.00mL sample of this stock solution is added to

62. ## chemistry

A 2.500×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3mL . The density of

63. ## chemistry

Which of the answer choices correctly describes a solution that has less of a solute dissolved in it than the maximum amount possible for a given temperature and pressure? colloidal solution saturated solution supersaturated solution unsaturated solution

64. ## Chemistry

Confused on these, please explain or show work for the answer if you can. :) 1. What is the morality of a water solution that freezes at -0.633°C? 2. What is the freezing point of a solution that contains 1.99 g of a molecular solute of molar mass 58.5

65. ## CHEMISTRY

Dye of iodine is prepared by dissolving in ethanol , and 1% ( one percent ) of this solution contains 10 g of solute in 1000 g of solution 1) how many grams of solvent is there in the solution ? 2) how many moles of solute ( I2) is there? 3) what is the

66. ## chemistry

how do you find the mass solute(g), GFM(g/mole), moles of solute, volume of solution, and molarity of solution (M), of CaSO(4)? *how would i solve this set by set? * what are the formulas?

67. ## chemistry

I collected questions from my book which I don't understand plz help me I am stuck plzz.!!!!!!!! Three different solutions containing the same solute at the same temperature are made to be saturated. Beaker 1 has 200.0 mL, beaker 2 has 500.0 mL and beaker

68. ## CHEMISTRY.

Lowering of vapor pressure is directly proportional to: a) Temperature b) Mole fraction of Solute c) Mole fraction of Solvent d) Amount of solution

69. ## Chemistry

When 3.15 g of a nonelectrolyte solute is dissolved in water to make 135 mL of solution at 21 °C, the solution exerts an osmotic pressure of 869 torr. What is the molar mass of the solute? What is the molar concentration of the solution? How many moles of

70. ## chemistry

What volume of solution would be needed to deliver the stated amount of solute? 237 milligrams of solute from a solution that is 32.0 ppm? answer in liters

71. ## chemistry

What volume of solution would be needed to deliver the stated amount of solute? 39.0 grams of solute from a solution that is 16.0 % m/v? (anwser in milliliters

72. ## chemistry

A solution contains 10.05 grams of an unknown covalent substance in 50.0 grams of water. The freezing point of this solution is (-) 3.16o C. What is the formula weight of the unknown compound? Below is what I tried, but don't know what to do next. Please

73. ## Chemistry

To illustrate the calculation, assume that 21.95 mL of a thiosulfate solution is required to reduce the iodine liberated by 20.85 mL of 0.0200M KIO3 and that 18.63 mL of the same thiosulfate solution reacts with the iodine replaced by 20.00 mL of an

74. ## chemistry

Can someone make sure that I am correct with my first solution? Also I need help with the 2nd problem. I am a little confused about where to begin. 1.) 1.7423g of potassium dichromate were placed in a 250.00 mL volumetric flask and water was added to the

75. ## Chemistry

Consider a solution containing 4.35 mM of an analyte, X, and 1.09 mM of a standard, S. Upon chromatographic separation of the solution peak areas for X and S are 3251 and 10075, respectively. Determine the response factor for X relative to S. F=? To

76. ## AP Chemistry

There is an unknown amount of unlabelled monoprotic acid in an unknown amount of water titrated with a sample with a solution of NaOH of unknown molarity. After adding 10.0 mL of NaOH, the pH=5.0. The equivalence point is 32.22 mL of NaOH. What is the Ka?

77. ## Chemistry

What is the molarity of the resulting saline solution when you mix 1 mole HCl with 1 mole NaOH? I'll provide some basic information that I know, but could somebody tell me how to get the answer using the data? The balanced reaction is as follows:

78. ## Chemistry

A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of

79. ## chemistry

A 1.147 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.690 grams of KI and 50.00 mL of a 0.00821 M KIO3 solution. The excess I3– was

80. ## chemisry

An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the di- luted NaOH solution. Answer in units of M

81. ## Chemistry

How do you calculate the concentration (ppm) if you have: the amount of total solution (60 ml) the amount of sample that is added to the solution (15 uL) the density (0.904 g/mL)

82. ## College Chemistry

You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured

83. ## Science

I need to calcuted the molarity from this 12.5 g of ethylene glycol antifreeze dissolved in o.100kg of water. Density of solution is 1.0 g/mL I know molarity if mole of solute / L of solution. I am confused on how to find the L of solution. Do I add 12.5

84. ## Chemistry

How do you calculate the concentration (ppm) if you have: the amount of total solution (in ml) the amount of sample that is added to the solution (in uL) the density (g/mL)

85. ## chemistry

Which of the following is NOT true for solutes and solvents? A. At least one solvent must be dissolved in a solute to make a solution. B. Solute concentration can be measured in terms of solute moles / solution volume or solute moles / solvent mass. C. A

86. ## chemistry

A compound was found to be composed of the following amounts of elements: 20.00% wt% C, 26.64wt% O, 46.65 wt%N, and 6.71wt%H. A 6.125 grams sample of this compound dissolved in 46.205 grams of water as a solution was found to have a freezing point of

87. ## Chemistry

calculate the final concentration if 4.0 L of 1.5 M NaCl and 2.0 L of 3.0M NaCl are mixed. I am confused about how to calculate the final concentration. We are currently working on solutions. I think first I need to divide the amount of the solution by the

88. ## Chemistry

A student weights 1.700 g of succinic acid and dissolves it in water in a 250.0 mL volumetric flask. A 25.00 mL sample of this solution is withdrawn and placed in a 125 mL Erlenmeyer flask, to which 5 drops of the acid-base indicator phenolphthalein is

89. ## Chemistry

A 0.4584 g sample of impure zinc chloride, ZnCl2, FW = 136.3 g/mole, was dissolved in water and excess silver nitrate was added to the solution. The mass of the dry silver chloride, AgCl, FW = 143.3 g/mole, produced was 0.8564 g. The balanced precipitation

90. ## Chemistry

when 5.0g of KOH is added to 100mL, of water, the temperature of the solution increases by 3 degrees celsius. Assume the density of the solution to be 1g/mL and specific heat capacity of the solution to be 4.184 J/g K. a. calculate the amount of heat

91. ## Chemistry

I don't know how to start this problem. Someone can help me please. One dm3 of a solution was prepared containing 0.0040 mole of Pb(NO3)2. The Ksp of PbCI2 for the existing conditions is 2.4 x 10^-4. From the list below, choose the smallest numbers of

92. ## Chemistry

Find the amount of mole solute in solution of concentration 2.5moldm^-3 and volume of 500cm^3 Hint to solve Amount = C x V

93. ## Chemistry

Calculate the pH after 0.016 mole of NaOH is added to 1.05 L of a solution consisting of 0.138 M HONH2 and 0.127 M HONH3Cl, and calculate the pH after 0.016 mole of HCl is added to 1.05 L of the same solution of HONH2 and HONH3Cl. (Assume that all

94. ## CHEMISTRY.

Lowering of vapor pressure is directly proportional to: a) Temperature b) Mole fraction of Solute c) Mole fraction of Solvent d) Amount of solution

95. ## Chem 2

When 3.89 g of a nonelectrolyte solute is dissolved in water to make 835 mL of solution at 26 °C, the solution exerts an osmotic pressure of 825 torr. What is the molar concentration of the solution? How many moles of solute are in the solution? What is

96. ## Chemistry

When 3.10 g of a nonelectrolyte solute is dissolved in water to make 755 mL of solution at 26 °C, the solution exerts an osmotic pressure of 821 torr. What is the molar concentration of the solution? How many moles of solute are in the solution? What is

97. ## Chemistry

Calculate the amount of solute needed to make the solution. I can't remember how to set these up. .50kg of a 18% (m/m) KOH solution