Number of results: 53,472
Chemistry
A sample of 8.00 L of NH3 (ammonia) gas at 22 degree Celsius and 735 torr is bubbled into a 0.500 L solution of 0.400 M (hydrochloric acid). The kb value for NH3 is 1.8 x 10^-5. Assuming all the dissolves and that the volume of the solution remains at 0.500L , calculate the pH...
Friday, April 24, 2009 at 12:52am by Linda
CHEMISTRY
Solution A has pH of 4.6 and solution B has a pH of 8.0 1- What is the (H3O+) in solution A? 2- What is the (OH-) in solution B ?
Thursday, June 3, 2010 at 8:56pm by Lynne
Analytical Chemistry
The question: The pH of a solution is defined as pH = -log[H3O+]. If the pH of a solution is 3.72(+/- 0.03), what is the [H3O+] and its absolute standard deviation? Answer: How would I carry this out? I know to find the hydronium concentration wouldn't i just take e^3.72? ...
Monday, January 28, 2013 at 10:16pm by James
Chemistry
Two Concept Questions for you: 1) Why is the concentration of a solution such as NaH2PO4 ignored when calculating the pH given Ka1, Ka2, and K3 values? 2) Given Pka1=3.13, Pka2=4.76, and Pka3 = 6.40, calculate the pH of lemon juice which is about 5% citric acid. --I know I ...
Tuesday, April 13, 2010 at 8:48pm by Chemistry Confused
chemistry
When excess solid Mg(OH)2 is shaken with 1.00 L of 1.2 M NH4Cl solution, the resulting saturated solution has pH = 9.30. Calculate the Ksp of Mg(OH)2 I am not sure where to even begin on this problem.
Sunday, March 21, 2010 at 2:56pm by Raj
Chem
calculate pH of the buffer solution prepared by mixing 10 mL of 1.5 M HCl with 100 mL of 0.1 M K2CO3 solution. For H2CO3: Ka1= 4.46 e^-7, Ka2= 4.69e^-11
Wednesday, November 12, 2008 at 10:52pm by Sam
chemistry
Write an equilibrium reaction for a buffer system made of the weak base, B, and its conjugate acid. If the buffer contains 1.05 M of B and 0.750M conjugate acid and has a pH of 9.50, what is the pH after 0.0050 mol HCl is added to 0.500 L of this solution?
Monday, April 9, 2012 at 11:35am by meme
Chem II
Can you use the Henderson-Hasselbalch equation to decide? pH = pKa + log [(base)/(acid)] pKa for NH3 is about 4.74. Calculate the pH of a 0.1 M solution of NH3, then add 0.1 mol NH4NO3 and see which way it goes.
Monday, April 14, 2008 at 6:04pm by DrBob222
Help Chemistry
Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the ...
Tuesday, December 7, 2010 at 11:01am by Jessica
chemistry
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at each of the following. (a) pH 7.7 (b) pH 9.6 (c) pH 11.3
Wednesday, March 27, 2013 at 10:35am by hannah
Chemistry
Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic acid=4.75) I got pH= 3.88 ...
Sunday, February 27, 2011 at 12:49pm by Jon
chemistry
Calculate the concentration in molarity of sugar in a solution made by dissolving 0.34 moles of dextrose (C6H12O6) in enough water to make 3.00 Liters of solution
Friday, December 2, 2011 at 12:59am by Seep
Chemistry
A solution is prepared by dissolving 50.0 g of pure HC2H3O2 and 20.0 g of NaC2H3O2 in 975 mL of solution (the final volume). what is the ph? What would the pH of the solution be if 50.0 mL of 0.900 M NaOH were added? What would the pH be if 30.0 mL of 0.30 M HCl were added to ...
Monday, November 12, 2012 at 8:39pm by Bella
Chemistry
If pH = 6.6, calculate the molar concentration of H^ + (aq) in the solution.
Wednesday, November 14, 2012 at 10:06pm by Josh G.
chemistry
Calculate the pH of a 2.5x10-5 M lithium hydroxide solution.
Wednesday, May 2, 2012 at 2:18am by Liz
Chemistry
I don't know why on earth I don't remember how to do this, but I can't, and it's so simple. Calculate [H+] and [OH-] of a solution with a pH of 9.7 Thank you.
Wednesday, June 15, 2011 at 2:06am by Anonymous
chemistry
calculate pH of 0.1M CH3COOH of 100ml of that solution?
Sunday, February 13, 2011 at 2:53am by kabelo
chemistry
calculate pH of 0.1M NH4^- of 100ml of that solution?
Sunday, February 13, 2011 at 2:52am by kabelo
chemistry
Calculate the pH of a 5.20 10-3 M solution of H2SO4.
Sunday, November 28, 2010 at 9:46pm by justin
chemistry
How much 6M HNO3 will be required to decrease the pH of 5000L solution of pH=9.6 to pH=3?
Friday, January 4, 2013 at 5:45am by vidya
Chemistry
You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 5.00 using only pure acetic acid, 3.00 M NaOH, and water. Calculate the quantities needed for each of the following steps in the buffer preparation. 1. Add acetic acid to ~400 mL of water in a 500 mL beaker. ...
Friday, September 28, 2012 at 2:33am by Kw1h
ChemB
A forming acid solution has a pH of 3.25. Which of these substances will raise the pH of the solution upon addition? Explain. A) HCl B) NaBr C) NaCHO2 D) KCl
Monday, March 12, 2012 at 2:12am by ALISON
chemistry
millimols HCl = 35 mL x 0.342M = ? mmols NaOH = 5 x 0.173 = ? Calculate each, determine the one in excess, calculate the amount in excess, then if acid pH = -log(H^+) or if basic then pOH = -log(OH^-) and convert to pH by pH + pOH = pKw = 14.
Wednesday, December 5, 2012 at 11:30am by DrBob222
chemistry
Calculate the pH of each of the following strong acid solutions. 0.697 g of HClO3 in 2.97 L of solution. so i convenrted grams to moles then moles/L to get M of HCl03 then i did -log of that cocentration and put htat as the ph. did i do something wrong? i got 2.415 but it was ...
Saturday, March 2, 2013 at 3:06pm by hannah
Chemistry
Calculate the concentration of H+(aq) and the concentration of OH-(aq) for the following solution with the following pH at 298K showing all your working. pH = 3.20
Sunday, April 29, 2012 at 4:52pm by JJ
AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:14pm by fernatesfsdf
AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:01pm by JIM
Chemistry
determine the pH of a solution made by mixing 8 ml of 1.10M acetic acid and 2ml 0.9 M sodium acetate solution. pKa for acetic acid CH3COOH is 4.745. Can someone please explain
Sunday, June 12, 2011 at 11:01pm by Max
chemistry
I assume you want the pH of the solution. pH = pKa + log(base)/(acid) Substitute and solve or pH.
Wednesday, October 24, 2012 at 8:20pm by DrBob222
CHEMISTRY
HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a strong acid (HNO3); therefore, it doesn't ...
Tuesday, February 27, 2007 at 11:05pm by CANDY
chem
First calculate the pH of the solution. pH = pKa + log [(B)/(A)] pH = 9.24 + log [.105/0.135] = 9.13. You really don't need that but it's nice to know the starting point. The slip in the pH you have as the minimum (9.00) and calculate base/acid ratio. 9.00 = 9.24 + log...
Monday, October 25, 2010 at 3:34am by DrBob222
Chemistry
0.0020 mole of HCl is dossolved in water to make a 2000ml solution. Calculate the molarity of the HCl solution, the H30, and the pH. The H30 is the same as the molarity of the HCl solution.
Wednesday, December 1, 2010 at 2:42pm by Susie
Chemistry
How many moles of NaOH must be added to 1.0 L of 1.4 M HC2H3O2 to produce a solution buffered at each pH? (a) pH = pKa mol (b) pH = 3.07 mol (c) pH = 5.15 mol
Sunday, December 5, 2010 at 3:22pm by justin
Chemistry
A titration is performed by adding .600 M KOH to 40.0 mL of .800 M HCl. Calculate the pH before addition of any KOH. Calculate the pH after the addition of 5.0 mL of the base. Calculate the volume of base needed to reach the equivalence point. What is the pH at the equivalence...
Friday, April 1, 2011 at 1:18pm by Summer
Chemistry
Calculate the pH after 0.14 mole of NaOH is added to 1.07 L of a solution that is 0.54 M HF and 1.15 M NaF, and calculate the pH after 0.28 mole of HCl is added to 1.07 L of the same solution of HF and NaF. 0.14 mole of NaOH 0.28 mole of HCl
Wednesday, March 13, 2013 at 2:46am by Margaret
Chemistry
A 25.0mL sample of a 0.100M solution of acetic acid is titrated with a 0.125M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added.
Monday, November 8, 2010 at 2:32pm by Amanda
chemistry
What is the pH of a solution made by adding grams of NH4Cl, to 550 mL of 0.205 M NaOH?
Wednesday, April 20, 2011 at 6:54pm by Tom
chemistry
What is the pH of a solution made by dissolving the 37 g of KOH in 500 mL of water, with no buffer in it?
Wednesday, March 9, 2011 at 12:24pm by Tayler
Chemistry
What volume of a 0.22mol/L hydrochloric acid solution is needed to cause the pH of 25.00mL of a 0.15mol/L lithium hydroxide solution to have a pH that s equal to 7.00
Saturday, February 16, 2013 at 9:42pm by Amy
Chemistry.
pH C ( dark green) pH : 8 d ( purple) pH : 3 Suppose u mix togather equal amounts of the solutions that produced the results of strip C and strip D , then test the pH of this new solution. What colo will the indicator paper be ? Explain.
Saturday, February 23, 2013 at 10:43am by Mia
Chemistry
Calculate the molarity of a solution made by dissolving 0.680 grams of Na2SO4 in enough water to form exactly 940 mL of solution. Please show me how to solve
Thursday, October 7, 2010 at 5:29pm by Veronica
chemistry
I have already posted this and never got a response, please help. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01...
Sunday, February 3, 2008 at 2:49pm by student
chemistry
The concentration of HNO3 in a solution is 3.50 10-6 M. What is the [H3O+] in the solution? _______M What is the [OH-] in the solution? ________ M What is the pH of the solution? What is the pOH of the solution?
Tuesday, December 21, 2010 at 8:26pm by jim
DrBob222 : need help with the problem
An unknown compound, X, is though to have a carboxyl group with a pKa of 2.0 and another ionizable group with a pKa between 5 and 8. When 75 mL of 0.1M NaOH is added to 100 mL of a 0.1M solution of X at pH 2.0, the pH increases to 6.72. Calculate the pKa of the second ...
Tuesday, September 11, 2012 at 12:55am by ron
Chemsitry
A chemist needs to make 50 mL buffer solution with a pH value of 7.25 using the acid/conjugate base pair of KH2PO4 and Na2HPO4 (which has an effective pKa = 6.86). The buffer solution needs to be made so that the total concentration of buffer is 0.10 M (that is, [acid] + [base...
Monday, April 2, 2012 at 11:39pm by Cassandra
chemistry
The concentration of NaOH in a solution is 7.00 10-6 M. What is the [H3O+] in the solution? _______________M What is the [OH-] in the solution? __________M What is the pH of the solution? What is the pOH of the solution? HELPP?? i don't understand any of this...
Wednesday, December 22, 2010 at 4:17pm by jim
Chemistry
Calculate the concentration of the hydronium ion([H3Ol+]) for a solution with the pH = 4.5
Sunday, March 25, 2012 at 12:27pm by Lisa
Chemistry
A solution is prepared by diluting concentration HNO3 to 2.0 M,Calculate PH.
Wednesday, November 23, 2011 at 12:12pm by Ethio
organic chemistry
calculate the pH of a 1.25 x 10^-3 M HNO3 solution
Monday, May 2, 2011 at 2:07pm by kathy
chemistry
Calculate the H3O^+ and OH^- ion concentrations in a solution that has a pH of 3.72.
Saturday, February 26, 2011 at 11:48am by Maria
Chemistry
Calculate the pH of a 0.250M solution of Sulfurous acid, H2SO3.
Friday, February 18, 2011 at 2:51am by Josh
chemistry
these is 0.1M HCl of 100ml of that solution in a beaker,calculate pH?
Saturday, February 12, 2011 at 5:24am by kabelo
Chemistry help plz
How to calculate the hydronuim ion cencentration of solution with a pH of 2.5?
Thursday, December 23, 2010 at 9:22pm by Tarkan
COLLEGE CHEMISTRY
Calculate the pH of a 0.052 NH4Cl aqueous solution
Tuesday, November 9, 2010 at 2:02pm by shanice
chemistry
The pH of a solution is measured to be 5.4. Calculate the following: a) [H3O^+] b)pOH c)[OH^-]
Monday, June 28, 2010 at 12:49am by Jay
Chemistry
Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2.
Tuesday, March 2, 2010 at 6:22pm by Saira
chemistry
Calculate the pH of a 0.35 M solution of dimethylamine, (CH3)2NH.
Monday, December 7, 2009 at 11:26pm by donna
Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks can someone please answer my ...
Thursday, May 5, 2011 at 12:38pm by Renee
Chemistry
First, the question I'm given is: What is the pH of a 1.0 L solution containing 0.25M acetic acid and 0.75M sodium acetate ( Ka for acetic acid= 1.8x 10-5) So I took the -log(1.8x10-5)= 4.74+log(.75/.25)= 5.22 pH But then I'm asked if .050 mol NaOH is added to the ...
Monday, April 8, 2013 at 7:01pm by Marcus
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
Sunday, November 11, 2012 at 6:29am by Elaine
Chemistry
calculate the ph of a solution that results from titrating 0.0500 moles of cyanic acid to the equivalence point with an equal number of moles of OH-, if the final volume of the solution is 150 ml ka= 3.50 * 10^-4
Friday, April 6, 2012 at 11:13pm by Tasneem
Chemistry
A few questions I don't really get and need to see the work for A 50.0 mL sample of 0.55 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.51 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 multiplied by 10-5. What is the pH of a ...
Thursday, April 22, 2010 at 1:07am by Dubs
chem
A sample of 7.80L of NH3 (ammonia) gas at 22 degrees and 735mmHg is bubbled into a 0.350L solution of 0.400M HCL(hydrochloric acid). The Kb value for NH3 is 1.8x10-5 Assuming all the NH3 dissolves and that the volume of the solution remains at 0.350L , calculate the pH of the ...
Thursday, April 23, 2009 at 5:40pm by tomi
chem
A sample of 7.80L of NH3 (ammonia) gas at 22 degrees and 735mmHg is bubbled into a 0.350L solution of 0.400M HCL(hydrochloric acid). The Kb value for NH3 is 1.8x10-5 Assuming all the NH3 dissolves and that the volume of the solution remains at 0.350L , calculate the pH of the ...
Wednesday, April 22, 2009 at 4:09pm by tomi
Chemistry
What is the pH of a solution made up of 50cm^3 of 1M Ethanoic Acid and 25cm^3 of 1M sodium ethanoate? Assume Ka for Ethanoic acid is 1.8 x 10^-5 mol dm^-3 I'm not quite sure how to do this. I was going to use the equation pH = pKa + log[A-]/[HA] but it doesn't seem to ...
Monday, February 16, 2009 at 4:02pm by Alice
Please Help CHEM
Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the ...
Tuesday, December 7, 2010 at 2:03pm by Jessica
chem II
at the beginning you have a "pure" solution of pyridine with Kb = ? ........BN + HOH ==> BNH^+ + OH^- I....0.370M...........0......0 C.......-x............x......x E....0.370-x..........x......x Kb = etc. Substitute into the Kb expression and solve for x = (OH...
Thursday, May 2, 2013 at 10:54pm by DrBob222
chemistry
acetic acid: 0.1 M 30ml hydrochloric acid 0.1 M 5 ml sodium hydroxide 0.1 M 15 ml Buffer + 5ml of: 1.91 ph ph (measured): 4:52 ph HOW DO I CALCULATE PH(CALCULATED)? AND ALSO IT SAYS SHOW YOUR CALCULATION FOR THE PH OF THE BUFFER BEFIRE AND AFTER THE ADDITION OF HCL? COULD YOU ...
Saturday, July 14, 2012 at 6:28pm by fenerbahce
Math
H+(conc) = 10^-pH So, in the first case, H+ = 10^-4 in the second case, the concentration of H+ = 10^-8 Subtract these two to find the difference, or divide the two to find a ratio expressing the change. A pH below 7 is acidic, a pH above 7 is basic, so increasing pH means the...
Wednesday, October 17, 2012 at 9:46am by Jennifer
Chem 1A
Help please! How many moles of NaOH must be added to 1.0 L of 3.0 M HC2H3O2 to produce a solution buffered at each pH? 1) pH= 3.78 2) PH= 6.52
Thursday, March 15, 2012 at 10:01pm by Mackenzie
chem
A sample of 7.80L of NH3(ammonia) gas at 22 degrees Celsius and 735torr is bubbled into a 0.350L solution of 0.400M HCl (hydrochloric acid). The Kb value for NH3 is 1.8x10-5. Assuming all the NH3 dissolves and that the volume of the solution remains at 0.350L , calculate the ...
Thursday, April 16, 2009 at 2:14pm by tomi
Chemistry
This is probably easier then my making it but... Calculate the ph of a forming acid solution that contains 1.35% forming acid by mass. Assume a density of 1.01g/ml for the solution.
Friday, February 24, 2012 at 6:36pm by L.Bianchessi
Chem 12
Okay, this is a two-part question and the unit is acids and bases. Ka for NH4 is 5.6 x 10^ -10 Kb for NH3 is 1.8 x 10^ -5 1. Determine the pH of a solution prepared by adding 0.0500 mole of solid ammonium chloride to 100mL of a 0.150 molar solution of ammonia. 2. If 0.0800 ...
Tuesday, March 27, 2007 at 12:21am by Kevin
Chemistry Very Urgent!!
A 0.035 M solution of a weak acid (HA) has a pH of 4.88. What is the Ka of the acid? HA ==>H^+ + A^- Ka = (H^+)(A^-)/(HA) pH = -log(H^+) You know pH. Convert that to (H^+). (H^+)=(A^-) so plug those into the expression for Ka. (HA) = 0.035 M - (H^+). Plug that in. ...
Monday, April 2, 2007 at 11:35pm by Paul
science
Calculate pH of 0.01 M CH3COONa solution if pKa of CH3COOH is 4.74.
Monday, January 7, 2013 at 6:49am by kartikaya
analytical chemisty
Calculate the pH and pOH of a 0.00002M solution of acetic acid.
Sunday, September 23, 2012 at 10:14pm by mary
chemistry
Calculate the pH of an Aqueous 3.8 x 10^-5 M solution of barium hydroxide. I need help.
Tuesday, August 21, 2012 at 5:24pm by Vincent
chemistry
Calculate the pH of a 0.87 M NaCN solution. Solve it exactly (no assume x=0.1)
Tuesday, March 20, 2012 at 2:33pm by Justin
chemistry
Calculate the pH of a 0.063 M (C2H5)2NH solution (Kb = 1.3 10-3).
Thursday, November 24, 2011 at 12:53am by melissa
Chemistry
Calculate the pH of a 0.053 M (C2H5)2NH solution (Kb = 1.3 10-3).
Wednesday, November 23, 2011 at 7:11pm by Kaleen
chemistry
A solution formed by dissolving an antacid tablet has a pH of 9.18. Calculate [H+].
Thursday, January 20, 2011 at 3:14am by jaycab
Chemistry
Sorry. "Calculate the pH for 0.10 mol/L aqueous solution of NaCl".
Sunday, May 2, 2010 at 4:20pm by Stuck
Chemistry
How do you calculate the pH, pOH, [H3O] and [OH] for a 0.067 M solution of sodium iodate
Monday, April 14, 2008 at 11:00pm by LT
Chemistry!
HB, pH=1 To neutralize 10cm3 it took 5.00cm3 NaOH 10cm3 of the solution HB are diluted with water to make 1 litre of solution. The pH of the new solution is 3. Show that HB is the strongest acid.
Tuesday, November 24, 2009 at 5:53pm by Anonymous
chemistry
HB, pH=1 To neutralize 10cm3 it took 5.00cm3 NaOH 10cm3 of the solution HB are diluted with water to make 1 litre of solution. The pH of the new solution is 3. Show that HB is the strongest acid.
Tuesday, November 24, 2009 at 2:29pm by Anonymous
High School Chemistry
10mL of 0.10M HCl is given. What is the pH? How many milliliters of 0.10M NaOH would be required to neutralize it? What is the pH of the neutralized solution? What would the pH of the solution be if you added 20mL of NaOH? Here's what I have so far: pH of HCl=-log(0.10M)= ...
Monday, March 21, 2011 at 12:58am by Becky
Chemistry
I am confused about why this is the answer to a practice problem I was given. (answer is c). Could someone explain why/why not for each answer? 2) Solution A is made from 1 L of water and 0.1 moles of Na(CH3COO), and Solution B is made from 1 L of water and 0.1 moles of Na2(...
Sunday, March 7, 2010 at 10:23pm by Trixie
Chemistry
The pH of an 0.0870 M solution of weak acid A is 2.20. The pH of an 0.0830 M solution of weak acid B is 4.07. The pH of an 0.0890 M solution of weak acid C is 5.13. Identify the three acids from among those listed below (the Ka values are listed in Appendix E of your textbook...
Friday, April 12, 2013 at 12:46pm by Maddie
chemistry
A buffer solution was prepared by mixing 442 mL of 0.181 M NaOCl and 139 mL of 0.421 M HOCl. Calculate the pH of the solution given that Ka (HOCl) is 3.2 x 10-8.
Sunday, March 18, 2012 at 7:39pm by cathy
chemistry
I have many questions. I have a test tuesday and need to get these problems done and understand them today because i am currently studying. I am in college and my professor has not emailed me back regarding solutions for the review problems she posted. Is it possible if you ...
Saturday, April 23, 2011 at 6:10pm by Sarah (C)
Chemistry
pH pH ( strip c : 8 ) dark green pH ( strip d : 3 ) purple - suppose u mix togather equal amounts of the solutions that produced the results of strip c and d , then test the pH of this new solution. What color will the indicator paper be? Explain .
Sunday, February 24, 2013 at 5:30am by Ruby
College Chemistry
1) The concentration of the aluminum ion in a test solution is 0.10M. Using the Ksp for aluminum hydroxide (3. x 10^-34), calculate the concentration of hydroxide needed to precipitate aluminum hydroxide. From the concentration of the hydroxide, calculate the pH of the ...
Thursday, April 1, 2010 at 8:44pm by Zach
chemistry
Calculate the concentration (% W/V) of NaCl solution that was made by dissolving 15.0 g of sodium chloride in enough water to make 300.0 mL of solution.
Saturday, October 29, 2011 at 3:41pm by Chemistry Chick
chemistry
Hi DrBob222, this is regarding my Determining Ka of Acetic acid lab I talked about on April 5, 2008. Refer to the volume of NaOH on your graph from question 2. Calculate half this volume and on your graph, find the pH when the solution was half neutralized. did you get a pH in...
Sunday, April 6, 2008 at 9:07pm by Sarah
Chemistry
A solution is prepared by diluting 65.0 mL of 0.175 M methylamine, CH3NH2, to a total volume of 225 mL. Calculate the pH of the diluted solution. Kb (CH3NH2) = 4.40 x 10-4
Sunday, June 26, 2011 at 11:11pm by Mallory
chm
Calculate the PH OF A SOLUTION prepared by mixing 15.0mL OF 0.50 M OF NaOH AND 30.0mL OF 0.50 M BENZOIC ACID SOLUTION?( Benzoicacid is monoprotic and its dissociation constant is 6.5*10^-5)
Wednesday, March 31, 2010 at 4:23pm by ami
Chemistry
H20SO4(aq)-> 2H+(aq) + SO4 2- (a) Calculate the hydrogen ion concentration (in mol 1-1) in this solution. Show steps and explain your reasoning Also what is the pH of the sulfuric acid solution nearet whole number You don't have any numbers. Sulfuric Acid (H2SO4) is...
Friday, March 2, 2007 at 12:33pm by Adam
chemistry
Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 2.1 x 10-2 Ka (HX-) = 7.3 x 10-8 Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 9 x 10-5 Ka (HX-) = 5.3 x 10-11
Sunday, March 11, 2012 at 6:59pm by Anonymous
chemistry
1)Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 2.1 x 10-2 Ka (HX-) = 4.5 x 10-8 2)Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 5.3 x 10-5 Ka (HX-) = 5.3 x 10-11
Friday, October 21, 2011 at 8:41pm by yahn
chemistry
1.Does a pH of 8.6 describe a solution with a higher or lower hydronium ion concentration compared to a neutral solution? Is such as solution called acidic or basic? 2. Compared to a neutral solution, would you expect an acidic solution to have a higher or lower pH and a ...
Thursday, May 2, 2013 at 7:43am by alex
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