Q: Calculate the pH of a solution that is 0.56 M HC3H5O3 and 1.28 M NaC3H5O3. I used the H-H equation for this and got this so far: HC3H5O3 acid NaC3H5O3 base pH = pKa + log([NaC3H5O3]/[HC3H5O3]) = -log(Ka of

46,116 questions
1. chemistry

Q: Calculate the pH of a solution that is 0.56 M HC3H5O3 and 1.28 M NaC3H5O3. I used the H-H equation for this and got this so far: HC3H5O3 acid NaC3H5O3 base pH = pKa + log([NaC3H5O3]/[HC3H5O3]) = -log(Ka of HC3H5O3) + log(1.28/0.56) = -log(1.4*10^-4) +

asked by . on March 18, 2019
2. Chemistry

Find the ratio of the volumes of NaC3H5O3 soloution to HC3H5O3 (lactic acid) required to prepare a buffer with a pH of 3.90. the solutions are equal in molarity. Ka = 1.4 x 10-4 for HC3H5O3. ratio = ________ mL of NaC3H5O3 per mL of HC3H5O3

asked by Bill on February 22, 2017
3. Chemistry

.12M Lactic Acid (HC3H5O3, Ka=1.4x10^-4) is mixed with .10M NaC3H5O3 to form 1.00L solution. A. Calculate the pH of the solution after the addition of 50.0mL of 1.00M NaOH. B. Calculate the pH of the solution after the addition of 120.0mL of 1.00M NaOH.

asked by Emma on March 28, 2010
4. chemistry

Lactic acid, C3H6O3, is found in sour milk. A solution containing 1.00g NaC3H5O3 in 100.0mL of 0.0500M C3H6O3 has a pH= 4.11. Calculate the Ka of lactic acid

asked by Lauren on April 14, 2011
5. chemistry

How much NaC3H5O3 (in grams) is needed to create a 1000 ml volume of Ringer’s lactate solution?

asked by Jeff on September 8, 2011
6. Bio

How much NaC3H5O3 (in grams) is needed to create a 1000 ml volume of Ringer’s lactate solution?

asked by Joe on September 6, 2011
7. biology

How much NaC3H5O3 (in grams) is needed to create a 1000 ml volume of Ringer’s lactate solution?

asked by Jeff on September 8, 2011
8. Biology

How much NaC3H5O3 (in grams) is needed to create a 1000 ml volume of Ringer’s lactate solution

asked by Nicole on September 9, 2011
9. science: chemistry

How many moles of NaOH must be added to 1.0 L of 2.6 M HC3H5O3 to produce a solution buffered at each pH? 1)pH= 4.28 2)pH=pKa

asked by Julie on July 23, 2015
10. chemistry

A lactic acid/lactate ion buffer solution contains 0.43M HC3H5O3 and 0.90M C3H5O3-. The value of lactic acid is 1.4*10-4 calculate the pH of this buffer

asked by jennifer on June 16, 2015
11. Chemistry

A lactic acid/lactate ion buffer solution contains 0.19 M HC3H5O3 and 0.78 M C3H5O3-, respectively. The Ka value of lactic acid is 1.4*10^-4. Calculate the pH of this buffer.

asked by Lynne on June 5, 2010
12. Chmeistry

A lactic acid/lactate ion buffer solution contains 0.19 M HC3H5O3 and 0.78 M C3H5O3-, respectively. The Ka value of lactic acid is 1.4*10^-4. Calculate the pH of this buffer.

asked by Lynne on June 5, 2010
13. chemistry

Lactic acid, HC3H5O3(aq) is a weak acid that gives yougurt its sour taste(Yeeeeecccckkk). Calculate the pH of a 0.0010 mol/L solution of Lactic acid. The Ka for lactic acid is 1.4 x 10^-4

asked by Geroge B. on April 5, 2008
14. Ap Chemistry

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.038 M NaOH. (a) hydrobromic acid (HBr) (b) lactic acid (HC3H5O3) (c) sodium hydrogen chromate (NaHCrO4)

asked by Halah Warner on February 19, 2018
15. Chemistry

An 0.0284 aqueous solution of lactic acid is found to be 6.7% ionized. Determine Ka for lactic acid. HC3H5O3 + H2O H3O^+ + C3H5O3^- Ka =? Thanks.

asked by Sev on August 10, 2009
16. chemistry

Lactic acid, HC3H5O3(aq) is a weak acid that gives yougurt its sour taste(Yeeeeecccckkk). Calculate the pH of a 0.0010 mol/L solution of Lactic acid. The Ka for lactic acid is 1.4 x 10^-4 For Further Reading chemistry - DrBob222, Saturday, April 5, 2008 at

asked by Sarah on April 6, 2008
17. 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

asked by Jake on October 29, 2012
18. chem

NaC3H5O3 is needed to create 1000mL volume of ringers lactate with 6.5 ph

asked by debra on September 11, 2011
19. Chemistry

An 8 Molar (aqueous) solution contains H2O and HNO3. The solution has an S.G. of 1.24 at 25oC. HNO3 is a strong acid that completely dissociates in water. a) Calculate the mass of I Litre of solution. b) Calculate the mass concentration (g/L) of HNO3 in

asked by Dodes on November 3, 2017
20. 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

asked by EMMANUEL on June 6, 2018
21. Chemistry

A is a solution of trioxonitrate (v)acid, HNO3 of unknown concentration.B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25 cm3 portion solution B required an average of 24.00cm3 of solution A for neutralization using 2drops

asked by Ogbaji on June 6, 2018
22. chemistry

A) A solution was prepared by dissolving 1.113 g of MgCl2 into water and made up to 50.0 ml, calculate the molar concentration of the solution. B) A 250.0 ml of 0.50 M solution of Na3PO2 solution was prepared by diluting 2.5 M of stock solution. Calculate

asked by henry39 on December 24, 2016
23. chem

. (a) A solution was prepared by dissolving 1.4295 g of magnesium chloride (MgCl2) into water and made up to 25.0 mL, calculate the molar concentration of the solution. (3 marks) (b) A 250.0 mL of 0.50 M solution of sodium phosphate (Na3PO4) solution was

asked by lightning on October 13, 2016
24. chemistry

A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH

asked by jaycab on January 20, 2011
25. 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!

asked by Jones on September 8, 2012
26. 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!

asked by Jones on September 8, 2012
27. Chemistry

A 1X Phosphate Buffered Saline solution was prepared by adding 1.44g of Na2HPO4 and 1.44g of H2PO4- to 800mL of water. Additional components were dissolved in the solution: 8g of NaCl, 0.2g of KCl and 0.24g KH2PO4. The resulting buffer solution had a pH of

asked by Nicole on April 28, 2015
28. chemistry

A is a solution of trioxonitrate(v) acid, HNO3, of unknown concentration. B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25cm3 portions solution B required an average of 24.00cm3 of solution A for neutralization, using

asked by oward on May 24, 2016
29. Chemistry

A solution is prepared by mixing 8 mL of .2 M Fe(NO3)3, 10mL of .001 M NaSCN, and 7 mL of .1 M HNO3 a. calculate the concentration of Fe3+ in the solution b. calculate the SCN- in the solution

asked by Anonymous on February 20, 2011
30. chemistry

a 500ml stock solution of NAOH has a purity of 70% and a density of 1.9g/ml. calculate the concentration that would be in a 1L solution. calculate the molarity. What volume would we have to take to prepare 250ml of a solution of 0.1 mol/l

asked by helen on March 12, 2016
31. 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

asked by Jason on May 24, 2015
32. 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

asked by Jason on May 24, 2015
33. Chem I

Calculate the concentrations of hydronium and hydroxide ions in a solution prepared by dissolving 0.345g of solid NaOH in enough water to make 225mL of solution. Also calculate the pH and pOH of the solution.

asked by Natalea on November 15, 2010
34. chemistry

A solution of 220mL of 0.200M Koh is mixed with a solution of 120mL of 0.240M NiSO4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3.Calculate the molarity of all ions left in the solution?

asked by anonymous on October 9, 2011
35. Chemistry

A solution of 220mL of 0.200M Koh is mixed with a solution of 120mL of 0.240M NiSO4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3.Calculate the molarity of all ions left in the solution?

asked by anonymous on October 9, 2011

A solution of 220mL of 0.200M Koh is mixed with a solution of 120mL of 0.240M NiSO4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3.Calculate the molarity of all ions left in the solution?

asked by anonymous on October 9, 2011
37. Chemistry

A solution of magnesium chloride, MgCl2, is prepared by dissolving 19.0g of MgCl2 in 250 mL OF water. a.) Calculate the weight percent of magnesium chloride in solution. b.)The denstiy of the above solution is 1.05 g/mL. Calculate the molarity of the

asked by Josh on October 24, 2012
38. chemistry

Calculate the pH values and draw the titration curve for the titration of 500 mL of 0.010 M acetic acid (pKa 4.76) with 0.010 MKOH. Calculate the pH of the solution after 490 mL of the titrant have been added. Calculate the pH of the solution after 500 mL

asked by Crystal on February 3, 2017
39. chemistry

Calculate the pH values and draw the titration curve for the titration of 500 mL of 0.010 M acetic acid (pKa 4.76) with 0.010 MKOH. Calculate the pH of the solution after 490 mL of the titrant have been added. Calculate the pH of the solution after 500 mL

asked by Jasmine on January 31, 2017
40. Molality

An aqueous solution contains 8.7% NaCl by mass. 1. Calculate the molality of the solution. 2. Calculate the mole fraction of the solution.

asked by Kyle on January 30, 2010
41. 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

asked by Jessie on April 25, 2010
42. Chemistry

Solution x has a pH of 4.35. Solution y has 10- times high [OH-] compared to solution x. Solution z has a pH 4.0 units higher than that of solution x. calculate the ration of [H3O+] between solutions x&y and between x&z. What is the pH of solutions y and

asked by mary on March 19, 2013
43. chemistr

10g of nacl were added to 10ml of water. he resulting solution was diluted to be a final volume of 250ml. Calculate the molarity of the solution. My calculation 10g/58g/mol = 0.173M 0.173M/025L =0.689M Given the density of the solution is 0.9864g/ml.

asked by Fai on December 25, 2012
44. Chemistry

The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.

asked by Hilavidpreet on March 17, 2010
45. chemistry

A 2.5 g sample of NaOH (Mw = 40.00) was dissolved in water to give a solution of final volume 250 cm3. (i) With reasons, state whether NaOH is a strong or a weak base. Give the conjugate acid of NaOH and decide whether this conjugate acid is acid, alkaline

asked by LUx on April 21, 2013
46. chemistry

a solution was perpared by dissolving 4.765 g of AlCl3 in enough water to give 250 mL of AlCl3? a. how do you calculate the molarity of the solution b. how do you calculate the osmolarity of the solution

asked by Anonymous on October 5, 2011
47. Chemistry

You have 3.00 L of a 2.37 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO3(aq) called solution B. You mix these solutions together, making solution C. Calculate the concentration (in M) of Na+ ions in solution C.

asked by tina on May 6, 2011
48. chemistry

2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find the [H+] and the percent ionization of nitrous acid in this solution. b. Write the equilibrium expression and calculate the value of Ka for the weak acid. c. Calculate the pH of the

asked by bob on March 25, 2012
49. chemistry

Q.1 What will be the pH at the equivalence point during the titration of a 100 ml 0.2M solution of CH3COONa with 0.2M of solution of HCl?(Ka = 2*10^-5) Q.2 Aniline behaves as a weak base.When 0.1M,50ml solution of aniline was mixed with 0.1M,25ml solution

asked by gaurav on March 27, 2010
50. ap chemistry

for the following, mix the equal volumes of one solution from group I with one solution from group II to achieve the indicated pH. calculate the pH of each solution. Group I: .2M NH4Cl, .2M HCl, .2M C6H5NH3Cl, .2M (C2H5)3NHCl Group II: .2M KOI, .2M NaCN,

asked by hannah on February 9, 2012
51. Chemistry

A solution of ethanol has a concentration of 4.613 mol/L at 20ºC. The density of the solution is 0.9667 g m/L.. Calculate the molality of the solution..please show the solution..thanks a lot

asked by Syam on July 5, 2014
52. Chemistry

A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this

asked by Paul on January 31, 2011
53. 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

asked by Jessica on November 26, 2011
54. AP Chem

I had to do an experiment to calculate the enthalpy of solution of Epsom salts. I'm stuck on how to calculate the amount of the reactant in moles. Here's some preliminary data: 37.58 g of Epsom salts in the solution Molar mass of solution: 246.48 g/mol I'm

asked by Arianna on December 20, 2012
55. CHEMISTRY

A STUDENT STUDYING THE FE+3- HSCN equilibrium put into a test tube 10.00ml of 2.00 x 10-3 M Fe(NO3)3 with 10.0 mL of 2.00 x 10-3 M HSCN.THE H+ in the resulting solution was manteined at 0.500.By spectrophotometric analysis of the equilibrium solution, the

asked by da on September 18, 2011
56. Chemistry

This is a question I am presently doing right now which I found in my homework. I am quite sure that in (a) I have to use the Hasselbach equation though I am not sure how to work it out. If anyone knows any of the answers, and how you got to them, please

asked by Matthias on September 29, 2012
57. Chemistry

This is a question I am presently doing right now which I found in my homework. I am quite sure that in (a) I have to use the Hasselbach equation though I am not sure how to work it out. If anyone knows any of the answers, and how you got to them, please

asked by Matthias on September 29, 2012
58. Chemistry

A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this

asked by Paul on February 1, 2011
59. Chemistry

A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this

asked by Paul on January 31, 2011
60. Chemistry

A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this

asked by Paul on February 1, 2011
61. chemistry

Hi, The problem is: "Calculate the concentration of OH- and the pH value of an aqueous solution in which [H30+] is 0.014M at 25C. Is this solution acidic, basic, or neutral?" I have calculated the OH- concentration to be: 7.1 X 10^-14 When I calculate the

asked by LaurenM on March 30, 2011
62. chemistry

1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the solution? 2) A 0.25 M solution of a monoprotic acid, HA, has a pH of 2.54. What is Ka for this acid? The dissociation of HA is: HA + H2O H3O+ + A- (Hint: write the expression for pH) 3 A

asked by nicki on December 9, 2012
63. Chemistry

1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*

asked by JUNDY on March 10, 2015
64. chemistry

3. A solution is made by dissolving 5.00 g of impure sodium hydroxide in water and making it up to 1.00dm3 of solution. 25.0 cm3 of this solution is neutralized by 30.0 cm3 of hydrochloric acid of concentration 0.102 mol/dm3. a) Calculate the number of

asked by gasana on April 18, 2017
65. 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

asked by Anonymous on September 20, 2015
66. chemistry

An aqueous solution is made using 137g of diluted to a total solution volume of 1.30L .Calculate the molarity.molality and mass percent of solution.*assume a density of 1.08g/ml for the solution..

asked by noor on July 28, 2012
67. chemistry

Calculate the following quantity: Volume in mL of 21.4 M cobalt(II) chloride solution that must be diluted with water to prepare 17 mL of an 51.5 M solution. Calculate to 0 decimal places and do not include units. Also, do NOT use scientific notation.

asked by Ocsar on September 14, 2014
68. chemistry

A STUDENT STUDYING THE FE+3- HSCN equilibrium put into a test tube 10.00ml of 2.00 x 10-3 M Fe(NO3)3 with 10.0 mL of 2.00 x 10-3 M HSCN.THE H+ in the resulting solution was manteined at 0.500.By spectrophotometric analysis of the equilibrium solution, the

asked by Christina on September 29, 2012
69. College Chemistry

1) A 25mL sample of the .265M HCI solution from the previous question is titrated with a solution of NaOH. 28.25mL of the NaOH solution is required to titrate the HCl. Calculate the molarity of the NaOH solution. 2) A 1.12g sample of an unknown monoprotic

asked by Jessica on October 25, 2010
70. Chem

A solution is made by dissolving 26.9 g of NaOH in approximately 450 mL of water in a volumetric flask. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to total 500 mL of solution. Calculate the pH of

asked by Anonymous on February 27, 2013
71. Physical Chemistry HELP!!!!!

A solution of the sugar mannitol ( molar mass 182.2 g/mol ) is prepared by adding 54.66 g of mannitol to 1.000 kg of water. The vapor pressure of pure liquid water is 17.54 torr at 20o C. Mannitol is nonvolatile and does not ionize in aqueous solution. a.)

asked by Lan on October 14, 2006
72. vapor and osmotic pressure

A solution of the sugar mannitol ( molar mass 182.2 g/mol ) is prepared by adding 54.66 g of mannitol to 1.000 kg of water. The vapor pressure of pure liquid water is 17.54 torr at 20o C. Mannitol is nonvolatile and does not ionize in aqueous solution. a.)

asked by Amy on October 12, 2006
73. AP CHEM

It was found that 39.9 mL of this diluted solution solution was needed to reach the stoichiometric point in a titration of 7 mL of a phosphoric acid solution according to the reaction 3KOH(aq) + H3PO4(aq) ! K3PO4(aq) + 3H2O(L) Calculate the molarity of the

asked by Ankit on September 26, 2013
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

asked by titration on October 7, 2008
75. General Chemistry

Starting out with 50 mL of 0.20 M NaHCO3, calculate how many mL of 0.50 M NaOH solution to add to make 100 mL of approximately 0.10 M (total) buffer solution with a pH of 10.35. By adding NaOH, some of the NaHCO3 gets converted to the conjugate Na2CO3.

asked by Lucy on April 3, 2012
76. CHEMISTRY

1. What is the vapor pressure at 25°C of a solution of 1.20g of nephtalene C10H8 in 25.6g of benzone C6H6? The vapor pressure of pure benzene at 23°C is 86.0mmHg the vapor pressure of naphthalene can be neglected. Calculate the vapor pressure lowering of

asked by N COMAS on March 20, 2013
77. chemistry

Calculate the pH of 0.3 M HCl solution. Calculate the pH when 100 mL of a 0.5 M solution of NaOH are added to 300 mL of the HCl solution.

asked by Anonymous on July 2, 2016
78. chemistry

Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 ´ 10-4 Formic acid, HCHO2, 1.7 ´ 10-4 Lactic acid, HC3H5O3, 1.3 ´ 10-4 Propionic acid, HC3H5O2, 1.3 ´ 10-5 Benzoic acid, HC7H5O2, 6.3 ´ 10-5 Which of the following is the weakest

asked by michael on May 26, 2010
79. Chemistry

1) What is the vapor pressure at 25°C of a solution of 1.20g ofnephtalene C10H8 in 25.6g of benzone C6H6? The vapor pressure of pure benzene at 23°C is 86.0mmHg the vapor pressure of naphthalene can be neglected. Calculate the vapor pressure lowering of

asked by N comas on March 19, 2013
80. chemistry

the following titration data were collected: a 10 mL portion of a unknown monoprotic acid solution was titrated with 1.12340 M NaOH and required 23.95 mL of the base solution for neutralization. calculate the molarity of the acid solution calculate the

asked by Doss on October 25, 2011
81. Chemistry

25.0 mL of a NaCl solution (concentration unknown) was found to react with 20 drops of the chloride test solution from the PU Chloride Test Kit. Calculate the mass of NaCl (in grams) in this solution. Calculate the mass of NaCl required to prepare 0.250 L

asked by kt on October 3, 2010
82. Chemistry

A solution is prepared by dissolving 0.56 grams of benzoic acid (HC6H5CO2, MM = 122.12 g/mol, Ka = 6.4 X 10-5) in enough water to make 1.0 L of solution. Calculate the pH of this solution at equilibrium. 2. Calculate the pH of the system in Question 1 when

asked by meow on March 26, 2019
83. 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

asked by lucy on April 25, 2013
84. science

A solution of trioxonitrate(V) acid contained 0.67g in 100cm^3. 31.0cm^3 of this solution neutralized 2.5cm^3 of a sodium trioxocarbonate(IV) solution. calculate the concentration of the trioxocarbonate(IV) solution.

asked by Anonymous on November 23, 2018
85. science

A solution of aqueous ammonia contains 28.0% NH3 by mass. the solution has a density of 0.898g/mL. calculate the volume of this solution required to make 425mLof 0.320M NH3 solution.

asked by luke on November 18, 2016
86. Chemistry

A solution contains 15 g non-volatile non-electrolyte solute C6H14O6 dissolved in 500 g of water at 40 c. Calculate (A)Vapor pressure of the solution. (B)Boiling point of the solution. (C)Freezing point of the solution.

asked by Yeneta on September 1, 2012
87. chemistry

Calculate the molar concentrations for each of the following solutions: A)1.5g NaCI in 100 ml solution B)1.5g K2Cr2O7 in 100 ml solution C)5.55g Na2SO4 in 125 ml solution D)20g MgBr2 in 250ml solution

asked by twynna on February 20, 2011
88. chemistry 1046

A.Determine the pH of the solution. a solution that is 1.17% HCl by mass (Assume a density of 1.01 g/mL for the solution.) B. Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of

asked by Anonymous on July 3, 2012
89. chemistry

calculate the volume(ml) of a 0.215M KOH solution that will completely neutralize each of the following? a) 2.50ml of a 0.825M H2SO4 solution b) 18.5ml of a 0.560 M HNO3 solution c) 5.00mL of a 3.18 M H2SO4 solution

asked by Connie on April 28, 2011
90. Chemistry- Drbob-help

I have placed the answer I got please help. A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 870mL

asked by Paul on February 9, 2011
91. Chemistry

An aqueous KNO3 solution is made using 73.4g of KNO3 diluted to a total solution volume of 1.86 L. Calculate the molarity of the solution. (Assume a density of 1.05 g/ml for the solution.)

asked by Anna on January 29, 2013
92. Chemistry

1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*

asked by JUNDY on March 10, 2015
93. Chemistry

1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*

asked by JUNDY on March 10, 2015
94. 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

asked by cheri on September 19, 2012
95. 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

asked by Maria on October 18, 2013
96. 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

asked by Gabriella on September 11, 2013
97. chemistry

I. 1) Calculate the pH of the following solution: 0.1 M HF + 0.2 M NaCN Given: pKa for: HF/F- = 3.2 HCN/CN-= 9.4 2) Calculate the pH of the solution that results upon mixing 20.0 mL of 0.2000 M HCI with 25.0 mL of: a) distilled water c) 0.13 MNaOH e) 0.23

asked by abd on February 18, 2013
98. chemistry

SALT HYDROLYSIS 1.) Calculate the pH of a 0.24M sodium formate (HCOONa) solution. Kb=5.9x10^-11. 2.) Calculate the pH of 0.25M pyridium chloride (C5H5NHCl)solution. Ka=5.9x10^6.

asked by jaycab on January 20, 2011
99. Chemistry

Calculate the pH of a 5.90 10-3 M solution of H2SO4 I have tried doing this as pH=-log[H+] and also by multiplying the Molarity by two because there are two hydrogens and then doing the -log but both ways have gotten me the wrong answer is there something

asked by Ashley on March 5, 2012
100. chemistry

Calculate the boiling point elevation of a solution containing 22.8 g of glucose (C6H12O6) dissolved in 672.0 g of water. Calculate the freezing point depression for the same solution.

asked by mandy on February 28, 2010