Saturday
April 19, 2014

Search: Calculate the pH of 0.10 M aqueous solution of each of the hydrochloric and acetic acids: Complete the following table.

Number of results: 109,863

chemistry
the Ph of a solution of HCl in water is found to be 2.50. what volume of water would you add to 1.00 L of this soltuion to raise the PH to 3.10? I think I'm supposed to use the formula C1V1=C2V2 but where would i get the concentrations from?
Tuesday, August 4, 2009 at 9:43pm by Sevwerl

Chemistry: Freezing point
An aqueous solution is prepared by dissolving 1.08 g of human serum albumin, a protein obtained from blood plasma, in 50.0 mL of water. The solution has an osmotic pressure of 0.00770 atm at 298 K. What is the molar mass of the albumin? Answer: 6.86 x 10^4 g/mol
Monday, February 25, 2013 at 2:29am by JJ

Chemistry!! Please Help!
1.43 x 10^-6 ix correct. NaA(aq) ==> Na^+ + A^- The anion hydrolyzes in water solution to produce a pH of 9.65 A^- + HOH ==> HA + OH^- Kb = Kw/Ka = (HA)(OH^-)/(A^-) You know pH. Convert that to pOH and convert that to OH^-. That = (HA) also. You know (A^-) from the ...
Friday, February 6, 2009 at 3:38pm by DrBob222

Chem II
Calculate the pH and percent ionization for the solution made up of 0.035 M NH3 and 0.015 M NH4Br.
Monday, April 14, 2008 at 6:05pm by Ken

chemistry
Calculate the ionization constant, Ka, of phenol (HC6H5O), a weak acid, if a 0.25 M solution of it has a pH of 5.24.
Monday, November 15, 2010 at 6:07pm by Audrey

Chemistry
14-pH=pOH=14-10.5=3.5 pOH=-log[OH-]=3.5 10^-(pOH)=10^-(3.5)=OH concentration in M 4.40L*(OH concentration in M)= moles of OH moles of OH*(39.997 g/mol)= mass of NaOH needed mass of NaOH needed Since 15% is 0.15g of NaOH/g of solution, solving for g of solution mass of NaOH ...
Sunday, March 17, 2013 at 1:58pm by Devron

chemistry
How do you calculate the solubility at 25°C in grams per liter of silver iodide in an aqueous solution that is 0.15 M inpotassium iodide and 0.25 M in ammonia.
Friday, April 20, 2012 at 4:08am by Lisa

chem--need help, please!!!
Ka for benzoic acid, C6H5COOH, 6.5x10^-5. Calculate the pH of solution after addition of 10.0, 20.0, 30.0, and 40.0 mL of 0.10 M NaOH to 40.0 mL of 0.10 M Benzoic acid. PLEASE CHECK MY ANSWER!!!!! My answer is: Moles acid = 0.040 L x 0.10 M = 0.0040 Moles base = 0.010 L x 0.10...
Wednesday, October 20, 2010 at 12:33pm by Andy

chemistry......plz help
A solution is prepared by dissolving 10.00g of a monobasic salt in a total volume of 1.00litres. Th pH of this solution was measured at 13.07 and a conductivity experiment determined that this salt was completely ionized in solution. What is the molecular weight of this ...
Tuesday, March 24, 2009 at 7:21pm by tomi

chemisrty
what is the concentration of [H+} in molars, millimolars, and micromolars for a solution of pH 5? In case you need this information: milli= 10^-3 micro=10^-6 Thank you.
Saturday, February 2, 2008 at 12:47pm by alex

Chemistry
What is the pH of a 0.0054 molal solution of C2H2O4. First ionization constant K1= 6.5 x 10-2, second K2= 6.1 x 10-5.
Wednesday, March 24, 2010 at 10:06pm by James

Chemistry DrBob
its two sorry the whole thing that i wrote didn't show up again. What is the pH of the solution created by combining 2.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? Here is the chart that i am supposed fill out: mL ...
Thursday, May 1, 2008 at 4:53pm by Amy

CHemistry
you want to measure the rate of change of pH? Not knowing what you are doing, the simple answer is to put a pH indicator in the solution and proceed with the change process, monitoring pH vs time.
Wednesday, November 2, 2011 at 9:59am by bobpursley

chemistry
The only way I know to do this is to calculate the buffer capacity of each, then compare them. The buffer capacity is the number of moles of a strong acid or a strong base that causes 1.00 L of the buffer to undergo a 1.00 unit change in pH. So you calculate the pH of the ...
Sunday, December 12, 2010 at 5:28pm by DrBob222

Chemistry Damon
1g of mixture of na2c03 and k2c03 was made upto 250ml is aqueous solution . 25ml of this solution was neutralized 20ml of hcl of unknow concentration. The neutralized solution required 16.24ml of 0.1N AGN03 for precipitation. Calculate a) the k2c03 is mixture b) conc of hcl in...
Sunday, January 12, 2014 at 1:04pm by Ken Hung

CHEMISTRY HELP PLEASE!!!
The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu^2+(aq,1.0M)|Cu(s) what is the pH of the solution if Ecell is 375 mV? I first got .65 as my pH, but it said that it was wrong. ...
Saturday, March 30, 2013 at 9:33pm by clara

Chemistry PLEASE HELP!!!
'A buffer is prepared by mixing a 100.omL of a 0.100 M NH3 solution with a 0.200M solution of NH4CL solution and making the total volume up to 1.000L of water. What is the volume of NH4Cl solution required to achieve a buffer at ph=9.5? Ka of NH4=5.6x10^-10. The textbook says ...
Tuesday, December 11, 2012 at 12:14am by jemima

Chemistry
(a)What is the pH of a solution made by combining 200 mL of 0.1 M Lactic Acid with 300 mL of 0.075 M sodium lactate? (b) If 20 mL of 0.4 M HCl is added to the solution from (a) what is the resulting pH?
Tuesday, January 28, 2014 at 10:12pm by Anonymous

science grade 10
The (aq) stands for aqueous solution, and FeSO4 can either be named duretter or iron (+2) cation sulfate.
Thursday, November 5, 2009 at 12:07am by Emily

GENERAL CHEMISTRY
CALCULATE THE pH AND HYDROLYSIS IN 0.10 M AlCl3 SOLUTION.Ka = 1.2 X 10-5 FOR [Al(OH2)6]+3,OFTEN ABBREVIATED Al+3.TELL WHETHER pH IS ACID OR BASE.GIVE IONIC EQUATION. Help us a little by telling us how much you know to do and exactly what you don't understand about the problem...
Sunday, July 29, 2007 at 11:16am by SHAWN

chemistry
Think ammonia, NH3. NH3 + HOH ==> NH4^+ + OH^- Kb = (NH4^+)(OH^-)/(NH3). You've probably solved 100 problem where you know pH of a NH3 solution and you calculate (NH3). (CH3)3N does EXACTLY the same thing. (CH3)3N + HOH ==> (CH3)3NH^+ + OH^- Write Kb expression, look up ...
Sunday, March 28, 2010 at 5:25am by DrBob222

chemistry
pH = 6 = (H^+) = 1 x 10^-6M and OH^- = 1 x 10^-8 You want pH = 7 = (H^+) = 1 x 10^-7 and OH^- = 1 x 10^-7 In 1 L you have 1 x 10^-8 moles and you want 1 x 10^-7 moles so you must add 1 x 10^-7 - 1 x 10^-8 = 9 x 10^-8 mols and that times 6.022 x 10^23 OH^- ions/mole = number of...
Tuesday, September 21, 2010 at 10:21pm by DrBob222

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
Friday, November 23, 2012 at 4:18pm by Boo Boo

chemistry
Find the pH of a 0.010M solution of NH4ClO4 and the pH of a 0.010M solution of NH4C2H3O2.
Saturday, April 18, 2009 at 3:05pm by Hannah

Chemistry
A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0, 1, 5, 9, 9.9, 10, 10.1, and 12 mL.
Wednesday, November 14, 2012 at 9:25am by Missy

Chemistry
The secret to acid/base problems is to recognize what you have produced in the problem and determine the pH from that. A buffer solution is prepared by mixing the weak base ammonia (Kb=1.77x10^-5) with ammonium chloride. The concentration of NH3 is 0.10M and that of NH4Cl is ...
Saturday, May 15, 2010 at 2:10pm by DrBob222

chemistry
A 10.0 mL sample of 3.00 M KOH(aq) is transferred to a 250.0 ml volumetric flask and diluted to the mark. It was found that 38.5 ml of this diluted solution was needed to react the stoichimetric point in a titration of 10.0 mL of a phosphoric acid, H3PO4, solution. The ...
Saturday, June 20, 2009 at 12:16am by dan

Chemistry
Isn't 1.0*10^-3.5 the same as ] 10^-3.5? Punch in 10 on your calculator, raise it to the power of -3.5. I get 3.16E-4. So pH = -log(3.16E-4) = -(-3.5) = 3.5 Or you could remember that is 10^-pH. 10^-3.5.
Thursday, April 28, 2011 at 12:07am by DrBob222

Help Please! Science
maybe you want the math. pH=- log(H+) or H+=10^-ph for stomach, H+=10^-1.5 for tomatoes H= 10^-4 making a ratio, ratio= 10^(-1.5+4)=10^2.5 which is 750
Sunday, January 27, 2013 at 10:51pm by bobpursley

Chemistry
3) The pH of a buffer solution made out of 0.20mol/L hydrofluoric acid and 0.30mol/L sodiumfluoride is the same as a buffer solution that is made out of 0.10mol/L of acetic acid and 0.15mol/L of sodium acetate. HF: pH = 3.14 + log(0.3/0.2) = 3.33 HAc: pH = 4.75 + log(0.15/0.1...
Saturday, December 8, 2012 at 2:54pm by DrBob222

Chemistry
What is the pH of a solution prepared by mixing 10 mL of 0.10 M NH3 and 5.0 mL of 0.24 M NH4+. Assume Ka(NH4+) = 5.56 x 10^-10
Sunday, November 11, 2012 at 4:57pm by Liz

chemistry
Ignoring activities, determine the molar solubility of copper (I) azide (CuN3) in a solution with a pH of 10.83. Ksp (CuN3) = 4.9 × 10–9; Ka (HN3) = 2.2 × 10–5.
Thursday, March 21, 2013 at 3:43pm by Jackie

Chemistry Help Please!!!
1) Boric acid, H3 BO3, is a triprotic acid that dissociates in three reactions. The first dissociation step is: H3BO3 ⇌ H^+ + H2BO3^-, K(a1) = 7.3 x 10^-10; the second dissociation step is: H2BO3^- ⇌ H^+ + HBO3^-2, K(a2) = 1.8 x 10^-13; and the third dissociation ...
Monday, February 17, 2014 at 6:48pm by Mello

chemistry
Adding acid will make it more acid; pH will go down. Adding base will make the solution more basic; pH will go up. Adding water will make the solution more dilute and it will change the pH somewhat (a little more basic making pH go up); how much depends upon how much water is ...
Monday, January 24, 2011 at 10:58pm by DrBob222

Chemistry
Calculate pH from the Henderson-Hasselbalch equation to give you the initial pH. Then to that buffer you add 2.50 mL x 0.150 M HCl to 100 mL. That will add 0.000375 moles HCl. That will increase the mole CH3COOH by that amount and decrease moles CH3COONa by that amount. ...
Sunday, April 11, 2010 at 11:44pm by DrBob222

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 magnesium chloride ...
Wednesday, October 24, 2012 at 8:22pm by Josh

chemistry
What is the pH of the solution created by combining 1.90 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH with HCl pH with HC2H3O2 1.90 ? ?
Sunday, July 11, 2010 at 8:46pm by Sara

Chemistry
I misspoke. I thought the sulfate and fluoride were given but they are not. So you need to calculate the solubility BaSO4 ==> Ba^+2 + SO4^-2 Ksp = (Ba^+)(SO4^-2) = 1.1 x 10^-10. If we let Ba^+2 = S, then SO4^-2 = S and S^2 = 1.1 x 10^-10. Solve for S = 1.05 x 10^-5 M which ...
Monday, April 26, 2010 at 10:17pm by DrBob222

chemistry
A) solve for the number of grams of Ca2+ ion in a solution prepared by adding 1 gram of calcium oxalate powder to 100 mL at pH 9. (B) explain what happens to the dissolved Ca2+ calculated before if you reduce the pH of this solution to 2.
Monday, February 10, 2014 at 2:32pm by naresh

chemistry
Please judge my answer: Question: 24 mL of 0.39 mol/L acetic acid is titrated with a standardized 0.33 mol/L KOH solution. Calculate the pH of the solution after 17 mL of the KOH solution has been added. Assume the Ka of acetic acid is 1.8 x 10-5. Answer: The equation for this...
Tuesday, April 15, 2008 at 5:00pm by Abigail

Chemistry, #3
Thallium hydroxide is a strong base used in the synthesis of some organic compounds. Calculate the pH of a solution containing 2.55 g TIOH per liter. Sorry! I'm having a really hard time with this acid/base stuff! TlOH is a strong base as the problem says. Do it just as you ...
Saturday, August 4, 2007 at 4:47pm by Taasha

chem
Calculate the mole fraction of the solute in the following aqueous solution: a) .112M C6H12O6 (d=1.006g/ml). b) 3.2% ethanol, by volume (d=.993g/ml); pure CH3CH2OH, d=.789g/ml
Friday, February 4, 2011 at 7:46pm by emerald

chemistry
The question asks, "Butanoic acid has a partition coeff of 3.0 when distributed b/t water and benzene. Find the formal concentration of butanoic acid in each phase when 100 mL of 0.10 M aqueous butanoic acid is extracted with 25 mL of benzene at pH 10.00." I know that the ...
Sunday, November 15, 2009 at 8:35pm by Anonymous

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
Phenol (abbreviated HOPh) is a weak acid with a Ka= 1.29 X 10^-10. What is the pH of a mixture made by mixing 100.0 ml of a 0.700 M solution of phenol with 70.0 ml of a 1.00 M solution of NaOH? Help please and please show work... I'm so confused.
Tuesday, May 12, 2009 at 8:21pm by Chelsea

Chemistry 102
For a question like “calculate the pH of an aq.solution that is 1.0 M CH3COOH and 1.0 M CH3COONa, how do you know to write the equation like this: CH3COOH + H2O => H3O+ + CH3COO- and not like H3O+ + CH3COO- => CH3COOH + H2O for the ICE chart. This would switch the ...
Monday, May 3, 2010 at 11:32am by Nick

chemistry
A buffer solution contains 0.200 M NH3 and 0.250 M NH4Cl. What is the pH of the buffer solution after the addition of 10.0 mL of 0.100 M NaOH to 50.0 mL of the buffer? Kb for NH3 is 1.8 x 10-5.
Tuesday, October 26, 2010 at 9:25pm by Brett

chemistry
Let's let HPh equal phenol with H representing the hydrogen that ionizes and Ph representing the remainder of phenol. HPh ==> H^+ + Ph^- Write the Ka expression. Ka = 1 x 10^-10 = [(H^+)(Ph^-)]/(HPh) Before the ionization (HPh) = 0.106 M. Before the ionization (H^+)=(Ph^-)=...
Thursday, January 10, 2008 at 7:22pm by DrBob222

chemistry
pH = -log(H^+) pH = -log(1*10^1) punch 1*10^1 into the calculator, hit the log key, the calculator returns 1, add the - sign and you have it. pH for 10^2 = -2.
Thursday, May 3, 2012 at 11:25am by DrBob222

Chemistry
Determine the partial pressure of oxygen necessary to form an aqueous solution that is 7.7 x 10-4 M O2 at 25oC. The Henry's Law Constant for oxygen in water at 25oC is 1.3 x 10-3 M/atm
Tuesday, February 7, 2012 at 9:56pm by Zoe

chemistry
pls help. A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0, 1, 5, 9, 9.9, 10, 10.1, and 12 mL.
Saturday, December 1, 2012 at 7:16pm by Joycelyn

chemistry
hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M NaOH Base (in mL) is ...
Monday, July 12, 2010 at 3:05am by THOMAS

Chemistry
The Ka values of H2CO3 are shown below. Ka1 4.6 10-7 Ka2 4.4 10-11 What is the pH of a 0.17 M solution of Na2CO3?
Monday, October 25, 2010 at 9:28pm by Kelly

Chemistry
How many grams of NaF should be added to 612 ml of 0.4 M HF (Ka = 6.8 x 10-4) to produce a buffer solution where pH = 3.10?
Friday, April 12, 2013 at 1:48am by Ashley

ap chem
I was absent for this info and im stuck. A)calculate the pH in an acid-base titration when 10.00mL o 1.000 m NaOH is added to 50.00 mL of 1.000m HNO2. Ka=6.0x10^-4 B) How many grams of NaC2H3O2 must be added to 500mL o 0.200m HAc to produce a buffer with pH=5? 1.8 x 10^-5 =Ka ...
Sunday, June 10, 2007 at 7:19pm by Just

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (a) Write a balanced chemical equation for the neutralization reaction upon which ...
Tuesday, November 27, 2012 at 11:08pm by sabrina

Chemistry
The boiling point of an aqueous solution is 102.16 C. What is the freezing point? Dr. Bob, If you happen to answer this question, I was the one that a question earlier about how to know what Kf constant to use [water vs benzene?] and i didn't notice that it was given in the ...
Friday, February 17, 2012 at 1:20am by Tracy

Chemistry
Calculate the pH of a solution that is 0.060 M in potassium propionate(C2H5COOK or KC3H5O2) and 0.085 M in propionic acid (C2H5COOH or HC3H5O2)
Thursday, October 28, 2010 at 1:47pm by Anonymous

chemistry
Calculate the pH after 0.15 mol of NaOH is added to 1.00 L of the solution that is 0.50 M HF and 1.01 M KF
Friday, March 25, 2011 at 4:42pm by kyle

Chemistry
10 mL of 0.1 HCl was added to 9mL of water. 10 mL of that solution was added to another 90 mL of water. The student diluted the sample as above 1 time(s). What is the pH of the solution?
Monday, April 7, 2014 at 5:13pm by Keyatta

Biochem
Assuming that the value of the equilibrium constant for the aldolase reaction Keq=6.43*10^-5 at pH=7 a.) What will be the equilibrium concentration of dihydroxyacetone phosphate (DHAP) if 1 mM of fructose-1,6-biphosphate is added to a buffered solution (pH=7) of aldolase? b.) ...
Wednesday, January 30, 2008 at 6:46pm by Obert

ThermoChemistry
Calculate the final temperature of solution when 10 g of oxalic acid, (COOH)2(s), is dissolved in 110.0 mL of water that is initially at 26 C. The enthalpies of formation of oxalic acid in the solid and aqueous phases are -826.8 and -818.8 kJ/mol, respectively. The heat ...
Friday, December 2, 2011 at 2:25pm by LaurenB

chemistry
the density of a certain aqueous solution is 1.17g/ml, and the solution is 3.57% by mass NaOH. how many mL of this solution would you need to use in order to prepare 100.0 mL of .150 M NaOH solution?
Monday, September 6, 2010 at 6:46pm by zahra

chemistry
What is the pH of the solution created by combining 11.40 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? Complete the table below: Note: Make simplifying assumptions, do not use the quadratic formula. What are the pH ...
Sunday, October 30, 2011 at 9:10pm by Billy

Chemistry
The pH at the beginning is pH = pKa + log(base)/(acid) Substitute pKa, base, and acid, and solve for initial pH. You have 100 mL 0.100M NH3 and 0.100M NH4Cl = 10 millimoles of each. You're adding 5.00 mL of 0.100M HCl = 0.500 millimols. .......NH3 + H^+ ==> NH4^+ + H2O I...
Thursday, December 5, 2013 at 12:26pm by DrBob222

chemistry
Calculate the pH of 3.9 10-8 M HNO3.
Sunday, November 28, 2010 at 9:47pm by justin

Chemistry
Calculate the ph of 10^-8 M (HCL).
Wednesday, June 29, 2011 at 1:05pm by gagan

Chemistry
A student begins with 25 mL of a 0.434 M solution of HI and slowly adds a solution of 0.365 M NaOH. 1. What is the pH after 15.00 ml of NaOH solution has been added? 2. What is the pH after 40 ml of NaOH solution has been added?
Monday, June 3, 2013 at 10:03pm by zac

chemistry
A new antibiotic drug has been developed for human oral administration. TECHNICAL DATA FOR ANTIBIOTIC AS FOLLOWS; pKa = 2.1; pH = 2.0 (stomach); pH = 6 (intestines) Will the drug dissociate in aqueous solutions as a weak or strong acid? Explain
Monday, March 19, 2012 at 11:13pm by ryan

Chemistry
pH=-logHconcentration Hconcentration=10^-pH a. 10^-6.66= 2.19E-7 c. 10^-13.17=1.70E-14
Tuesday, March 18, 2014 at 10:15pm by bobpursley

chem
Complete the table below: Note: Make simplifying assumptions, do not use the quadratic formula. What is the pH of the solution created by combining 1.00 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? table 1: mL NaOH=1.00 ...
Tuesday, May 1, 2012 at 5:20pm by Heather

chemistry
calculate the pH of a buffer solution containing 0.200M acetic acid, HC2H3O2, plus 0.150M sodium acetate. The dissociation constant for HC2H3O2 is 1.76 x 10-5 I dont think our instructor gave enough notes on these things Im kind of winging it from the book. Could you please ...
Friday, November 11, 2011 at 8:02pm by Monique

college chem
. Jack Daniels Tennessee whiskey is 40.00% ethanol by volume. However, % alcohol by mass is quite different from % by volume. The molality of ethanol in an aqueous solution that is 40.00 % ethanol by volume is 10.88 molal. A) Find the % ethanol by MASS, based on the molality. ...
Tuesday, March 9, 2010 at 11:11pm by josh

chemistry
The pH at the beginning of the titration is just the pH of a 0.2 M HF solution. b). moles HF = M x L = ?? moles NaOH = M x L = ?? Which is in excess. Subtract. If HF in in excess, you will have a buffer solution of HF and NaF. If NaOH is in excess the pH will be determined by ...
Saturday, November 6, 2010 at 5:04pm by DrBob222

chemistry
which of the following liquids have the highest freezing point? a- aqueous Fe(NO3)3 (0.030) b- aqueous glucose (0.050 m) c- aqueous NaI (0.030 m) d- aqueous NaI (0.010 m) e- pure water please explain the concept behind it as well thank you!
Monday, November 5, 2012 at 10:49pm by Ania

Chem
1) Which solution will have the lowest OH- A) Na2CO3 B) NaHCO3 C) NaCl D) NaHSO4 E) NH4Cl 2) Which solution will be the strongest base? A) Na2CO3 B) NaHCO3 C) NaCl D) NaHSO4 E) NH4Cl 3) Which aqueous solutions are acidic? A) Na2CO3 and NaHCO3 B) NaCl and NH4Cl C) NaHSO4 and ...
Saturday, April 5, 2014 at 9:33pm by Timothy

science/chemistry
thank you! What is the molar concentration of hydroxide ions in a solution with a pH of 6? Find the concentration of H ions first.. [H+]= antilog -ph Then, find [OH-] [OH-]= 1*10^-14/[H+]
Tuesday, June 5, 2007 at 6:04pm by Devon

Chemistry
Which would react faster with MeI in aqueous solution: OH- or Et3N? I know that the reaction in aqueous solution would be an Sn1 reaction and so steric hindrance wouldn't have such a great effect. I am not sure which is a better nucleophile out of OH- and Et3N. OH- is charged...
Tuesday, May 26, 2009 at 3:05pm by Alice

Chemistry
1.)Find the PH of a solution with 0.20M NH3 with 0.15M of NH4Cl. 2.)Find PH of a solution with a mixture of 200mL of 0.50M HCHO2 and of 100mL of .50M NaCHO2.
Tuesday, May 1, 2012 at 5:02pm by Chem help me!

AP CHEMISTRY
A solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x10^-10. (A) Assuming that the hydroxide is 1.0 x 10^-2 M, calculate ...
Wednesday, April 11, 2012 at 7:27pm by DAN

CHEM 136
A sample of 25.00 mL of 0.100 M HNO2(in a flask) is titrated with 0.150 M of NaOH solution at 25 degrees. 1) calculate the volume(Ve) of the NaOH solution needed to completely neutralize the acid in the flask. 2)calculate the pH for (a)the initial acid solution in the flask (b...
Tuesday, November 23, 2010 at 4:49pm by Jefferson

chemistry
How many grams of NH4Cl must be added to 0.490 L of 1.70 M NH3 solution to yield a buffer solution with a pH of 9.40? Assume no volume change. Kb for NH3 = 1.8 10-5.
Wednesday, October 26, 2011 at 7:36pm by kelly

Chemistry
A precipitate will be formed when an aqueous carbonic acid soution is added to what other aqueous solution? A. ammonium chloride B. calcium hydroxide C. Sodium Chloride D. Potassium carbonate E. Nitrous acid
Saturday, June 19, 2010 at 1:48pm by Ellie

Chem 100L
Calculate the molarity of an aqueous NaOH solution if 32.00ml of it is required to titrate .6789g of oxalic acid to a phenophthalein end-point. the balanced chemical equation is H2C2O4 + 2NaOH ---> Na2C2O4 + 2H2O
Sunday, December 2, 2012 at 3:40pm by Tammytha

Chemistry
Calculate the initial molarity of KNH2 and the molarities of K+, NH3, OH-, and H3O+ in an aqueous solution that contains 0.75 g of KNH2 in 0.255 L of solution. You may ignore the reaction of NH3 with water. I already found the initial molarity, but I am not sure how to find ...
Monday, February 22, 2010 at 7:18pm by Trixie

Chemistry
How many mL of a solution of NaOH with pH equal to 1.395 x 101 do you need to mix with pure water to obtain 399 mL of a final solution with pH equal to 9.066 ?
Tuesday, January 17, 2012 at 2:19pm by Summer

Chemistry
Use solution B to solve for the Ka of the weak acid. Use Ka from above to solve for the pH of solution A. That gives you the first 3 numbers of the combination. Use solution C and the Henderson-Hasselbalch equation to solve for the pH of that solution which will be last three ...
Tuesday, May 27, 2008 at 7:38pm by DrBob222

chem
I don't think so. Now that I see the question again, I'm wondering if this is a problem with two parts; i.e., the question is asking for the pH of 0.0515 M HCl and for the pH of a separate solution of 0.0762 M NaC2H3O2? And after noticing that there is no volumes listed for ...
Thursday, April 16, 2009 at 2:09pm by DrBob222

General Chem
What do you call a solution that is maid by mixing solid Na2S2O3 5H20 with NaOH? Also, what is the complete balanced equation for mixing the above solution with an aqueous solution of NaClO? Thanks anyone!
Wednesday, June 22, 2011 at 7:14pm by Mark

Chemistry
NH3 + HCl ==> NH4Cl moles NH3 = M x L = ?? moles HCl = M x L = ?? Determine from the moles you have which reagent is in excess, determine the molarity from M = mole/L and find pH of the resulting solution. I suspect NH3 is in excess and that will produce a buffered solution...
Sunday, February 13, 2011 at 11:32pm by DrBob222

chemistry (confirmation)
If the reverse reaction is favoured and it includes a solid as a reactant, the solid concentration is not going to increase as solids and liquids stay constant right? To determine which solution is most basics given [OH-] / [H30+], you take the -log and you compare it on the ...
Sunday, July 20, 2008 at 12:52pm by Xi

chemistry
solution The hydrogen ion concen.(H+),of the acid is 0.25moldm3 ie(H)=0.25 but ph=-log{H+} ie pH=-Log{0.25} =-log{2.5*10`} =-0.398+1=0.602 but pH+pOH=14 i.e 0.60+pOH=14 ^pOH=14-0.60 =13.40
Thursday, March 10, 2011 at 5:56am by peter onoriode

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (a) Write a balanced chemical equation for the neutralization reaction upon which ...
Wednesday, November 28, 2012 at 12:35am by sabrina: PLease someone help!

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (a) Write a balanced chemical equation for the neutralization reaction upon which ...
Wednesday, November 28, 2012 at 1:08am by sabrina: I am having difficulties with this!

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (1a) Write a balanced chemical equation for the neutralization reaction upon which ...
Wednesday, November 28, 2012 at 8:27pm by sabrina: Please help

CHEMISTRY
Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L-1 CH3CH2NH2 (aq) is titrated with 0.150 mol L-1 HI(aq) solution at 298 K. (1a) Write a balanced chemical equation for the neutralization reaction upon which ...
Wednesday, November 28, 2012 at 11:36pm by sabrina: Please help

chemistry
What is the pH of the solution created by combining 2.40 mL of the 0.10 M NaOH(aq) with with 8.00 mL of the 0.10 M HC2H3O2(aq)? So, here's my working so far: .00024 mol NaOH .0008 mol HC2H3O2 .0008 - .00024 = .00056 mol HC2H3O2 .00056mol / 0.0104L = .05385 M HC2H3O2 The Ka of ...
Monday, May 4, 2009 at 10:59am by Brandon

chem
an aq. solution(NaCl) made by using 133g diluted to a total solution volume of 1 L.Calculate the molarity, molality & mass % of the solution(density of solution = 1.08g/mL) [ans: M=1.92M, m=2.0m, 10.4 %] i need the calculation work bcus my ans is contradict from the real ans.
Thursday, July 21, 2011 at 11:36pm by lily

Titration
This is the titration of a strong base with a strong acid. Begin: 100 mL x 0.100M NaOH = 10 millimoles. millimoles HBr added = 1.00M x mL = ? .............NaOH + HBr ==> NaBr + H2O initial......10mmol...0.......0......0 added.................0 change........-0............ ...
Monday, January 23, 2012 at 3:46pm by DrBob222

Chemistry
see same question how many grams nitric acid HNO3 must be dissolved in 350 ml water to make a solution with pH of 4.5"? or "how many ml of a 4.2M nitric acid solution are required to make 500 ml of solution with pH of 2.9
Sunday, May 12, 2013 at 11:29am by kriti

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