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April 18, 2014

Search: Calculate the concentration of the HCl solution

Number of results: 48,868

Chemistry
I am confused about where I am going wrong here... Suppose that 1.331 g of impure barium hydroxide is dissolved in enough water to produce 250. mL of solution and that 35.0 mL of this solution is titrated to the stoichiometric point with 17.6 mL of 0.0935 M HCl(aq). What ...
Saturday, March 13, 2010 at 6:23am by Val

Chemistry
Suppose 49.6 mL of 0.242 M CoCl2 solution is added to 23.8 mL of 0.361 M NiCl2 solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive. I'm not sure what to do! Thank you!
Sunday, May 9, 2010 at 10:09pm by Michael

chem help w/ Lab
Weight of the mustard package Sample: 3.02 (g) Weight of the mustard package Solution: 33.3 (g) Trial #1 Trial #2 Trial #3 Weight of Mustard Package Solution Delivered (g) : 1.09 .948 .909 Weight of NaOH Solution Delivered (g) : .354 .304 .269 Concentration of NaOH : 7.48e-3 (...
Wednesday, October 17, 2012 at 3:19am by Den

Chemistry
I just tried that and it told me the answer was incorrect. It gave a hint saying In acidic solution, use the reaction given for the solvation of CaCO3 in acidic solution. Construct a concentration table that allows for the calculation of final concentration as if the reaction ...
Monday, March 11, 2013 at 11:05pm by Andrew

Chemistry
A solution of is prepared by adding 50.3ml of concentrated hydrochloric acid and 16.6ml of concentrated nitric acid to 300ml of water. More water is added until the final volume is 1.00L. Calculate (H+) (OH) and the PH for this solution. Hint concentrated HCL is 38% hcl by ...
Saturday, August 11, 2012 at 1:57pm by Fai

Chemistry: Molarity
4.82 mL of a 0.262 M NaOH solution reacts completly with 4.79 mL of HCl solution according to the balanced chemical reaction shown below: HCl (aq) + NaOH (aq) -> NaCl*aq) + H2O (I) What is the molarity of the HCl solution? 4.82 x (1L/1000 mL) = .00482L 4.79 x (1L/1000 mL...
Sunday, March 1, 2009 at 11:41am by Bob

chemistry
A solution is prepared by dissolving 25.0 g of ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.0 mL sample of this stock solution is added to50.0 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.
Tuesday, March 1, 2011 at 2:30pm by Anonymous

chemistry
A lab tech had accidentally set out 16M HCl for this experiment. How much ( in mL) 16M HCl is needed to make 450mL of a 3M HCl solution?
Monday, October 7, 2013 at 5:22pm by Christina

biology (Help please!!!)
1. If a student pours a solution of salt water on an elodea leaf, what is it an example of? 2.A child pours salt crystals on the body of a slug he finds in the backyard. Options are: high concentration, low concentration, osmosis, diffusion, hypertonic solution, and hypotonic ...
Sunday, October 20, 2013 at 11:54pm by Samantha

chem
A solution is prepared by dissolving 16.5 g ammonium sulfate in enough water to make 145.0 mL of stock solution. A 10.50 mL sample of this stock solution is added to 57.70 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution. NH4+
Saturday, November 3, 2007 at 11:32pm by mel

Chemistry(Please check, thank you)
For an experiment on the effect of a buffer solution, I need to calculate the expected pH of the buffer. I know that I have to make an amounts table and use the Hasselbalch equation to find the pH. For the first part, 0.10M HCl was added to a buffer. The first addition was 5 ...
Thursday, March 29, 2012 at 1:25pm by Hannah

Chemistry
Calculate the molarity of the concd HCl. 1.20 g/mL x 1000 mL x 0.37 x (1/36.5) = about 12 M or so but you do it exactly. Then mL x M = mL x M mL x 12 M = 2800 mL x 0.475 Solve for mL of the concd HCl solution.
Thursday, February 21, 2013 at 8:26pm by DrBob222

Chemistry
A 5.00-mL sample of an H3 PO4 solution of unknown concentration is titrated with a 0.1003 M NaOH solution. A volume of 6.55 mL of the NaOH solution was required to reach the endpoint. What is the concentration of the unknown H3 PO4 solution?
Monday, March 11, 2013 at 2:13pm by Amee

Chemistry
If 0.10 mol of Zn(s) is reacted to 150.0 ml of 1M HCl, what is the concentration of Zn+2 in the solution after the reaction is complete? Assume the solid zinc does not affect the volume.
Sunday, February 16, 2014 at 5:22pm by Linda

chem
A standard solution is prepared for the analysis of fluoxymesterone (C20H29FO3), an anabolic steroid. A stock solution is first prepared by dissolving 13.0 mg of fluoxymesterone in enough water to give a total volume of 500.0 mL. A 100.0 µL aliquot (portion) of this solution ...
Sunday, November 4, 2007 at 12:07am by mel

chemistry
A standard solution is prepared for the analysis of fluoxymesterone (C20H29FO3), an anabolic steroid. A stock solution is first prepared by dissolving 13.4 mg of fluoxymesterone in enough water to give a total volume of 500.0 mL. A 100.0-µL aliquot (portion) of this solution ...
Tuesday, November 26, 2013 at 10:42pm by quincy

chemistry
How would you calculate the concentration of an aqueous solution of Ca(OH2)that has a pH of 12.57.
Wednesday, April 14, 2010 at 11:22pm by kia

Chemistry
Calculate the concentration of the solution in mass percent: 32.3 mg KNO3 in 2.44g of H2O.
Tuesday, November 30, 2010 at 7:17pm by Kelsey G

Chemistry
Calculate the concentration of all species in a 0.15 M KF solution. Ka = 6.4 x 10-4 for HF.
Sunday, February 27, 2011 at 6:20pm by Brian

chemistry
how to calculate molar concentration of a 500 millimeter solution that contains 20 gram of CaBr2 ?
Sunday, June 3, 2012 at 3:24am by star

Chemistry
Calculate the pH of concentrated hydrochloric acid if this solution is 24.8 % HCl by weight and has a density of 1.16 g/mL.
Saturday, November 1, 2008 at 11:47pm by A.A

chemistry
Calculate the grams of solute needed to prepare each of the following. 55.0 ml of a 6.50 hcl solution.
Friday, November 2, 2012 at 11:03am by mary

physical science
plan,design and condact an investigation to find out whether the amount of heat produced will depend on an increase on the concentration of HCl when HCl reacts with an excess Zn.
Thursday, April 25, 2013 at 5:08pm by kholofelo

chemistry
it is found that 23.8 ml of 1 x 10^-3 M Sr(OH)2 is required to titrate 10.0 ml of an HCl soln. A) what is the concentration of the HCl soln? B) what is the pH of the HCl soln?
Tuesday, May 18, 2010 at 10:44pm by jared

Chemistry (Acids and Bases)
Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ? (How do we calculate this) There isn't enough information to work the problem here. (weak acid) = moles NaOH/volume weak acid used in the titration. All ...
Sunday, March 29, 2009 at 1:54pm by DrBob222

Chemistry
A solution of acetic acid having a concentration of about 0.2M is to be titrated using 0.200M NaOH. Select an indicator for the titration. what salt will the solution contain at the equivalence point? what is the approximate concentration of this salt at the equivalence point...
Saturday, May 15, 2010 at 2:00pm by Alison

Chemistery
An aqueous solution of calcium chloride contains 2 g of calcium chloride (molar mass 110.98 g mol-1) in 100 ml. Calculate the concentration of chloride ion in the solution any help their
Tuesday, January 20, 2009 at 11:22pm by Slaysliver

Chemistry Solubility help!!!!!!!!!
INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 NaOH (12.1 mL of HCl needed to titrate) Flask C: 0.025 NaOH (10.8 mL of HCl needed to titrate) Flask D: 0.0125 ...
Tuesday, March 26, 2013 at 5:51pm by Sally

Chemistry
Use PV = nRT and calculate n = number of moles HCl. Don't forget to change mL to liters and T to Kelvin. That will give you moles. The molarity = mols/L solution = moles/4.30 = ?? molarity of the final solution.
Saturday, February 14, 2009 at 4:58pm by DrBob222

chemistry
0.5123 g KHP sample was dissolved in about 25 mL of distilled water, and titrated to the phenolphthalein endpoint with 28.75 mL of a sodium hydroxide solution. Calculate the molar concentration of the hydroxide solution
Saturday, October 16, 2010 at 12:26am by Cynthia

chemistry
g)How many grams of agarose are needed to make 100 ml of 2.5% agarose solution?. h) Calculate the volume of buffer to which 500mL of 40 mM potassium chloride solution must be diluted to make a new concentration of 0.001M.
Tuesday, September 13, 2011 at 1:39pm by roshan

Chemistry
How do I do this problem, I am very confused on how to even begin: An aqueous solution contains 0.167 M ascorbic acid (H2C6H6O6) and 0.194 M hydroiodic acid. Calculate the ascorbate (C6H6O62-) ion concentration in this solution. [C6H6O62-] =? mol/L.
Saturday, April 28, 2012 at 5:49pm by Dan

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 solution 25.0mL 1.60M ...
Monday, October 29, 2012 at 1:48pm by Jake

chemistry
What will be the final pH value if you mix 50ml HCl (aqueous solution, pH=0.5) and 40ml NaOH (aqueous solution, pH=12). Hint: convert pH value to concentration of acids/base, then consider the neutralization reaction, then find out the resulting pH value. Please show me your ...
Thursday, April 4, 2013 at 11:44am by Anonymous

Chemistry
a)HCl --> H^+ + Cl^- HCl is 100% ionized; therefore, (HCl) = (H^+) = 0.8M pH = -log(H^+) = ?? b)to start. moles HCl = M x L = 0.800*0.040 = 0.032. moles KOH added in 5 mL = M x L = 0.600*0.005 = 0.003 ................HCl + KOH ==> KCl + H2O initial......0.032....0...
Friday, April 1, 2011 at 1:18pm by DrBob222

Chemistry
Hydrogen peroxide solution, H2O2(aq), is available with a concentration of 1.667mol/L. When diluted to a concentration of 0.25mol/L, the solution is used as a disinfectant. What volume of water should be added to 100 mL of the concentrated hydrogen peroxide solution to prepare...
Thursday, February 21, 2013 at 7:19pm by Lori

Chemistry
If a chemist titrates 120.0 mL of NaOH with a 5.0 M solution of HCl and requires 56.0 mL of the acid to reach the endpoint, what is the concentration of the NaOH?
Friday, February 17, 2012 at 12:20pm by Anonymous

Chemistry
If a chemist titrates 120.0 mL of NaOH with a 5.0 M solution of HCl and requires 56.0 mL of the acid to reach the endpoint, what is the concentration of the NaOH?
Friday, February 17, 2012 at 1:47pm by Spacy1996

chemistry
You transfer a 2M stock solution of Y into a container using a slightly wet pipet containing water drops. The concentration of the transferred solution Y has a ? (lower, higher, or same) concentration than(as) 2M.
Thursday, April 3, 2008 at 5:26pm by Un

goechemistry-science
i ppted out iron(111) form a solution and weighed the ppt. then dissolved the ppt in a solution and run in an aas and get the concentration. how can i get the percentage concentration of fe3+ given that it is from fe(oh)3
Tuesday, March 13, 2012 at 5:36am by didymus mupambo

science
50 ml of ZnSO4 solution was transferred to a mercury cathode and enough solid potassium nitrate is added to make the solution 0.1 M in KNO3. The electrolysis of Zn2+ is carried to completion of -1.3 V vs. SCE with the passage of 241 C of electricity. calculate the initial ...
Monday, November 5, 2012 at 4:45am by Maya

science
50 ml of ZnSO4 solution was transferred to a mercury cathode and enough solid potassium nitrate is added to make the solution 0.1 M in KNO3. The electrolysis of Zn2+ is carried to completion of -1.3 V vs. SCE with the passage of 241 C of electricity. calculate the initial ...
Monday, November 5, 2012 at 4:46am by Maya

Chemistry - titration lab
Hello. For my chemistry of solutions class, we had a titration lab where we titrated NaOH into an HCl + H2O mix. This was a preparatory titration for the next one consisting of the hydrolysis of ethyl acetate into acetic acid with H+ ions as a catalyst (in our case the HCl). ...
Tuesday, July 31, 2012 at 11:42am by Robertq

Chemistry
HCl + NaHCO3 ==> NaCl + H2O + CO2 You don't have enough information to answer the question. You have M HCl and that's all. You must have the volume of HCl if you are to calculate the grams NaHCO3. I might point out that this would not be a very good airbag as it would ...
Wednesday, May 29, 2013 at 5:23pm by DrBob222

chemistry
if BaSo4 was precipitated in solution contain 0.012 M NaCl and 0.002 M BaCl2 .calculate the sulfate concentration which is sufficient for saturate the solution with BaSo4 , if you now that the Ksp for BaSo4 equal to 1*10^-10 .
Tuesday, December 21, 2010 at 4:09pm by shahad

Chemistry
I have interpreted this problem differently than Bob Pursley. I think the problem states that 85 mL HCl and 89 mL NaOH WERE LEFT when the accident was discovered; therefore, we have added 100-85 = 15 mL HCl and 100-89 = 11 mL NaOH. Therefore, mmoles HCl added = 15 mL x 0.06 M...
Thursday, July 9, 2009 at 3:16am by DrBob222

chemistry
What is the concentration of HCl in a 250.0 mL sample of hydrochloric acid if 15.5 mL of 0.0100 M NaOH is needed to react with all the HCl?
Tuesday, February 22, 2011 at 6:51pm by Maddy

Chemistry
3.25g of zinc was added to 50cm^3 of a 4.0 molar dm^-3 HCl. When the reaction was completed the temperature rose by 28 degrees celcius. (a) Is the reaction exothermic or endothermic? (b)All the zinc dissolve in this reaction. How many moles of zinc reacted? (c) How many moles ...
Monday, March 24, 2014 at 9:20pm by Jessica

physics practical investigation
Plan,design and conduct an investion to find out whether the amount of heat produced will depend on increase on concentration of Hcl when Hcl reacts with an excess zn.
Monday, March 25, 2013 at 5:14am by Jossie

physical sciences
plan,design and conduct an investigation to find out wether the amount of heat produced will depend on an increase on the concentration of HCL when HCL reacts with an excess Zn
Sunday, April 28, 2013 at 5:17am by machata rilinde

Environmental Chemistry
Calculate the pH when the following volumes of 0.20 M LiOH are added into 50 mL of a 0.1 M HCl solution. Both LiOH and HCl are strong electrolytes. a) 0 mL b) 10 mL c) 24.6 mL d) 25 mL e) 25.6 mL f) 30 mL g) 40 mL
Tuesday, May 8, 2012 at 11:50am by Dauren

Chemistry
Because AgCl forms a complex ion with AgCl which makes it more soluble in acid HCl solution than it would be in neutral solution. AgCl + HCl ==> AgCl2^- There also are other complexes. (AgCl3^-2).
Thursday, April 29, 2010 at 12:52am by DrBob222

Chemistry
Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 5.3 g of iron are to be dissolved in 1.7 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?
Sunday, September 11, 2011 at 11:50pm by Dave

Chemistry
Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 6.5 g of iron are to be dissolved in 1.4 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?
Monday, September 12, 2011 at 3:12pm by BillyBob

chemistry
Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 5.4 g of iron are to be dissolved in 1.1 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?
Tuesday, September 13, 2011 at 5:25pm by Carolina

Chemistry
If 50.0mL of 1.60M HCl was added to 50.0mL of 1.80M NaOH, calculate the molarity of the resulting NaCl solution. (Hint: resulting solution has a volume of 100 mL)
Thursday, April 1, 2010 at 1:23am by Michelle

Chemistry
If 50.0mL of 1.60M HCl was added to 50.0mL of 1.80M NaOH, calculate the molarity of the resulting NaCl solution. (Hint: resulting solution has a volume of 100 mL)
Thursday, April 1, 2010 at 10:55am by Jen

chemistry
A 25.0 mL solution of HCl has been spilt. It took 21.8 mL of saturated 2.5 M NaOH to neutralise the acid. What was the molar concentration of the acid?
Wednesday, August 7, 2013 at 11:42pm by sarah

chemistry
a. How many moles of NaOH are present in 89.6 mL of 0.714 M NaOH? 6.40E-2 b. How many moles of HCl are present in a 30.0 mL sample that is neutralized by the 89.6 mL of 0.714 M NaOH? 6.40E-2 c. What is the molar concentration of the HCl solution described in part b of this ...
Wednesday, February 29, 2012 at 1:09am by krystal

Chemistry
Can i please get a formula to calculate the concentration of an acid when it reacts with a standard solution? ( preferably 0.1 M NaOH and viniger )
Thursday, August 5, 2010 at 10:20am by Daniel

Chemistry
Calculate the molarity (M) of a solution of the strong acid HNO3 if the hydroxide ion concentration is 2.17E-12 M.
Thursday, May 12, 2011 at 10:40pm by Anonymous

chem
calculate the concentration of all ions present in 58.7 mg NH4Br in 500 mL of solution
Thursday, April 11, 2013 at 8:17pm by celine

Chemistry
Calculate the H3O concentration if 100.0 ml of the .10M HNO3 solution is diluted to 1.0L with water?
Thursday, April 25, 2013 at 8:03pm by Kim

chemistry
Calculate the molarity (M) of a solution of the strong acid H2SO4 if the hydrogen ion concentration is 0.000244 M.
Thursday, October 10, 2013 at 1:03am by HELP ASAP PLEASE

chemistry
Calculate the molarity (M) of a solution of the strong base RbOH if the hydroxide ion concentration is 0.000309 M.
Thursday, October 10, 2013 at 1:02am by HELP ASAP PLEASE

science
how do you do this question An aqueous solution of calcium chloride contains 2 grams of calcium chloride ( molar mass 110.98 g mol-1) in 100 ml calculate the concentration of chloride ion (Cl-) in the solution
Thursday, January 22, 2009 at 5:01pm by Slaysliver

Chemistry
The standard solution were prepared by transferring exactly 1.00 mL, 2.00 mL, 3.00 mL, 4.00 ml, and 5.00 ml, respectively, of stock solution to clean 100 ml vol flads, diluting to the mark with FeCl3 solution, and then filling the aoorioruatekt kabeked cuvette. Calculate the ...
Sunday, February 3, 2008 at 11:03pm by Anonymous

Chemistry
Chester makes 1L of a 0.01M HCl solution and measure the pH. Burt then adds 5.80 g of sodium chloride to Chester’s solution and measures the pH. Calculate the difference between the two pH values obtained.
Friday, February 14, 2014 at 6:05pm by Anonymous

chemistry
How would I calculate the molarity of the resulting solution if 25.0mL of 1.50 M HCL solution is diluted to 500 mL. I know you have to change the milliliters to liters by dividing by 1000 and I know that M= Moles of Solute/Liters of Solute but after that I'm lost. Please help!
Friday, July 1, 2011 at 4:13pm by Daniel

chemistry
If you take three times as much NaOH as the volume of HCl, the NaOH must be 1/3 the concentration of the HCl. Now, 1/3 of .1M is NOT .03M It is closer to .033333M
Thursday, April 22, 2010 at 11:26am by bobpursley

chemistry
a student was asked to prepare 100.0 mL of 0.0200 M solution of HCL from 0.400 M solution of HCL. in order to do this he measured 5.0 mL of 0.400 M HCL with a graduated cylinder, transfered this amount to a 100 mL beaker, added 95 mL of deionized water measured with a ...
Tuesday, November 12, 2013 at 11:08pm by morgan

Chemistry please help!
Please help. I have no idea how to do these 4 homework problems. 1- How many milliliters of 0.140 M HCl are needed to completely neutralize 42.0mL of 0.106 M Ba(OH)2 solution? 2-How many milliliters of 0.123 M H2SO4 are needed to neutralize 0.250 g of NaOH ? 3-If 55.2 mL of ...
Monday, February 22, 2010 at 1:30pm by Robert

chemistry
For the titration of 50.00 mL of 0.1000 M ammonia with 0.1000 M HCl, calculate the pH (a) before the addition of any HCl solution, (b) after 20.00 mL of the acid has been added, (c) after half of the NH3 has been neutralized, and (d) at the equivalence point.
Wednesday, April 11, 2012 at 6:03am by chamy

Chemistry
Tartaric acid has two acidic (ionizable) hydrogens. The acid is often present in wines and precipitates from solution as wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 22.62 mL of 0.2000 M NaOH solution of titrate both ...
Monday, October 10, 2011 at 7:37pm by Destiny

science
25 ml sample of 0.150 m solution of aqueous trimethylamine is titrated with 0.100 M soultion of hcl. calculate the pH of the solution after 10.0ml,20 ml and 30.0 ml of acid have been added; pkb of (CH3)3 N =4.19?
Monday, April 19, 2010 at 6:17pm by Jake

Chemistry
A 5.00-mL sample of a sulfuric acid solution of unknown concentration is titrated with a 0.1401 M Sodium Hydroxide solution. A volume of 5.99 mL of the base was required to reach the endpoint. What is the concentration of the unknown acid solution? Write the neutralization ...
Monday, June 24, 2013 at 8:13pm by Steptim

Chemistry
If a researcher needs 0.50 L of 3.0 M nitrite buffer at pH 3.00, then she knows that the concentration of nitrous acid (conjugate acid) plus the concentration of nitrite anion (conjugate base) must equal 3.0 M. She must then calculate the amount of each that is necessary to ...
Monday, April 11, 2011 at 8:40pm by Mike

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. Okay the answer is 5.00%....however I keep getting 0.0500%....Why? and which one is the correct answer? Thanks for your help...
Saturday, October 29, 2011 at 4:30pm by Chemistry Chick

Chemistry
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution?
Saturday, July 9, 2011 at 6:35am by Jayne

Chemistry
How much 12 M HCl do you add to 1 L of water to obtain 0.2 HCl? Use this same approach to do the math for the dilution of 5.5 M of barium hydroxide solution to 0.5 M barium hydroxide solution.
Sunday, February 19, 2012 at 4:03pm by Amanda

Chemistry
How much 12 M HCl do you add to 1 L of water to obtain 0.2 HCl? Use this same approach to do the math for the dilution of 5.5 M of barium hydroxide solution to 0.5 M barium hydroxide solution.
Sunday, February 19, 2012 at 4:04pm by Amanda

please help meDr.Bob
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 50.00mL of water. ...
Sunday, September 23, 2007 at 4:05pm by claudia

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!
Saturday, September 8, 2012 at 4:52pm by Jones

Algebra
equal amounts: 2.5% if 3% solution is x times the 2% solution, then if the resulting concentration is y%, .02 + .03x = (1+x)*y You can see that if x=1, y=.05/2 = .025 = 2.5% If x = 3, .11 = 4y, so y = .11/4 = .0275 = 2.75% Makes sense, since the new concentration is 3/4 of the...
Thursday, December 29, 2011 at 9:51pm by Steve

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!
Saturday, September 8, 2012 at 5:08pm by Jones

Chemistry
NH3 + HCl ==> NH4Cl 5.5 kg = 5500 g Convert to moles. moles = grams/molar mass = ? 1 mole NH3 requires 1 mol HCl; therefore, moles NH3 = moles HCl. M HCl = moles HCl/L HCl. You know M HCl and moles HCl, solve for L HCl
Saturday, February 11, 2012 at 9:14pm by DrBob222

chemistry
If you add a metal piece to excess acid, what of listed factors below will increase, decrease, or have no impact on how fast a reaction happens? a) lower molarity (concentration) of a solution b) higher molarity (concentration)of a solution c) increase volume of a solution (...
Wednesday, May 22, 2013 at 10:08pm by K

chemistry
25ml of 0.05M of NaOH and the average volume of HCl is 17.7ml after titration and the concentration of HCl is 0.1028M. Find the [OH] eq (from titration). How do u solve this...
Wednesday, March 23, 2011 at 6:58pm by roshan

Chemistry
A solution with pH = 4 has 1. relatively high concentration of OH- 2. relatively low concentration of H3O+ 3. relatively high concentration of H3O+ 4. zero concentration of OH- Some of the answers people are giving me are confusing. I just need to know if it 1,2,3 or 4?
Saturday, October 22, 2011 at 7:26pm by nan

Chemistry
A stock solution was prepared by dissolving exactly 0.4000 g of pure ASA (180.16g/mol) in 10.00 mL of NaOH and heating the solution to a gentle boil. After cooling to room temperature, the solution was poured into a 250 ml volumetric flask and diluted to the mark with DI water...
Sunday, February 3, 2008 at 11:00pm by Anonymous

Chemistry
Need Help!! Describe how to make 2.5L of 0.1M HCL solution from 12M HCL concentrated solution and water. I got help earlier but still could not figure out the calculations. Please help, it has been a while since i took chemistry. Thank you soo much
Wednesday, August 29, 2012 at 1:08am by debbie

acid-base titrations
For each of the following circumstances, indicate whether the calculated molarity of NaOH would be lower, higher or unaffected. Explain your answer in each case. a.the inside of the pipet used to transfer the standard HCl solution was wet with water. mols HCl = L x M If pipet ...
Monday, April 21, 2008 at 10:22pm by DrBob222

Chemistry
yes. The problem in words works out this way. You have so many mols NH3 at the beginning. You had an excess of HCl which reacts with all of the NH3 and leaves extra HCl in the solution. The first thing you want to do is to find the how much excess HCl is there. You do that by ...
Sunday, February 2, 2014 at 1:49pm by DrBob222

Chemistry
A complicated work but do-able. NaOH + HCl ==> NaCl + H2O. I think one must decide where we are at the equivalence point. Since the M NaOH is twice that of the HCl, that means the HCl will take twice as much to neutralize the NaOH. So that 35 mL is made up of 2 mL HCl for ...
Sunday, May 2, 2010 at 11:52pm by DrBob222

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
Calculate the Ksp Ca(OH)2 25cm3 of a saturated solution required 11.45cm3 of 0.1mol/dm3 HCl for neutralization.
Monday, January 3, 2011 at 10:18am by Suha

chemistry
If you have all of the information posted, then 500 mL of the saturated solution of Ca(OH)2 must have used 0.10 x 0.050 L = 0.005 mols HCl. The reaction is Ca(OH)2 + 2HCl ==> CaCl2 + 2H2O. Therefore, mols Ca(OH)2 must be 1/2 of the HCl mols or 0.005/2 = 0.0025. From there ...
Tuesday, April 1, 2008 at 3:23pm by DrBob222

chemistry
Calculate the concentration, in percent by mass, of a refrigerant brine solution which is 4.03 M in NaCl with a density of 1.116 g mL-1.
Friday, November 9, 2007 at 8:44pm by keely

chemistry
Calculate the mass of silver nitrate needed to prepare a solution of concentration 0.01 moles per litre
Monday, April 4, 2011 at 10:45pm by Anonymous

AP CHEMISTRY
If a solution of HF (Ka = 6.8 10-4) has a pH of 3.42, calculate the total concentration of hydrofluoric acid.
Tuesday, February 14, 2012 at 5:17pm by Stanley3000

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