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April 20, 2014

Search: how many ml of 0.15 m naoh solution are required to neutralize 35.00 ml of 0.22 m hcl amp

Number of results: 42,405

chemistry
To make 10 mL of 25 mM sodium standard, what volume of 1 M NaCl stock should be used? 250 mL 2.5 mL 0.25 mL 0.5 mL None of these 400 mL
Thursday, February 24, 2011 at 11:16am by vivek

chemistry
30 ml of 0.1M sodium acetate and 15 ml of 0.1 M hydrochloric acid was mixed together. What is the pH of the resulting solution?
Wednesday, March 25, 2009 at 12:59am by Anonymous

chemistry
Calculate pH for strong base solution: 15.0 mL of 1.2010^−2 M Ca(OH)2 diluted to 460.0 mL
Sunday, February 26, 2012 at 6:49pm by jeff

chemistry
4.50% by mass means 4.50 g EtOH/100 g solution. The density is 1.00 g/mL; therefore, that becomes 4.50 g EtOH/100 mL. How much alcohol is contained in 355 mL of the beer? 4.50 g EtOH x 355 mL/100 mL = 15.975 grams EtOH. You get 1367 kJ for each 46 g EtOH according to the ...
Thursday, October 21, 2010 at 1:28pm by DrBob222

Chemistry: Dilution
mL x M = mL x M. 250mL x 0.20 M = mL x 1.0 M solve for mL of 1.0 M NaCl. Then ? mL of 1.0 M NaCl in a 250 mL volumetric flask, and make to the mark with water.
Thursday, June 4, 2009 at 7:08pm by DrBob222

Chemistry
Isn't a five fold dilution just making the solution more dilute by a factor of 5? So 2.15M/5 = 0.43M 75 mL x 0.43M = mL x 2.15 M Solve for mL of the 2.15M solution to use.
Monday, March 21, 2011 at 2:16pm by DrBob222

chemistry
Which one of the following will have the greatest number of moles of potassium ion: 10.0 mL of .10 M potassium hydroxide, 30.0 mL of 0.15 M potassium carbonate, or 25.0 mL of 0.080 M potassium phosphate
Sunday, July 31, 2011 at 11:29pm by lori

Chemistry
How much water must be added to 6 mL of a 0.05M stock solution to diltue it to 0.02M ? The answerI got is 15 mL. Is this correct? Thanks
Thursday, April 18, 2013 at 10:53pm by Shadow

chemistry
millimoles HNO3 = mL x M = 50.00 x 0.3M = 15 millimoles. mmoles KOH = mL x 0.6M = mL = 0, 0mmoles KOH mL = 15.5, 9.3 mmoles mL = 25.0, 15 mmoles mL = 40.0, 24 mmoles I'll do the 15.5 or 9.3 mmoles KOH added. ..........HNO3 + KOH ==> KNO3 + H2O initial...15......0........0...
Friday, December 2, 2011 at 6:50pm by DrBob222

Chemistry
Performing a gravimetric analysis of Ca2+. 25 mL of unknown [Ca2+} added to 25 mL of 0.15 (NH4)2C2O4 and 75 mL of HCl. Urea also added. H2NCONH2 + 3H2O --heat→ CO2 + 2NH4 + 2OH CaC2O4*H2O --> Ca2+ + C2O42- [Ca2+]unknown=0.06028 M <--0.0015433 moles of Ca2+/0.025 L ...
Monday, March 25, 2013 at 10:32pm by Anonymous

Chemistry
What is the molarity of a solution of Mg(OH)2 if the solution contains 1.35 g in exactly 100 mL of solution??? A 15.0 mL solution of H2SO3 is neutralized by 12.0 mL of a standradized 1.00M NaOH solution. What is the concentration of the H2SO3 solution?????? What volume of a 1....
Wednesday, December 12, 2012 at 12:24am by Tasha

chemistry
mL x M = mL x M 1000 mL x 6M = mL x 0.5M Solve for mL which gives th TOTAL volume needed.
Thursday, March 17, 2011 at 4:05pm by DrBob222

Chemistry
I finally caught on to what you're doing. Your error is you think (100 ml/4 ml) = 4 mL. It isn't. It is 4. The mL in the top cancels with the mL in the bottom to leave a unitless number of 4.00
Thursday, December 6, 2012 at 12:38am by DrBob222

chemistry dilution
This is a confusing problem. Here is another approach. We have a soln that is 200 ug/mL. We want 3 ug/100 uL. That is 0.003 ug/uL = 3 ug/mL Say we want to make 100 mL of this solution, then 3 ug/mL x 100 mL = 300 ug we need. 200 ug/mL x ?mL =300 ug ?mL = 300/200 = 1.5 mL; ...
Wednesday, February 27, 2013 at 8:54pm by DrBo222

Chem
A 50 ml sample of 0.025M AgNo3 is mixed with 15 ml of 0.04 M CrCl3. How many grams of AgCl will precipitate? Please show steps
Saturday, October 9, 2010 at 5:15pm by MAX

chemistry
How much of the water (in grams or mL) is consumed to produce 15 mL of the H2 gas? Use PV = nRT ; assume T = 298K, P = 1 atm
Thursday, December 1, 2011 at 11:29am by mook

Chemistry
Determine the sulfate ion concentrate in a solution prepared by diluting 15.00 ml of 0.115 M Y2(so4)3 with 35 ml of water?
Thursday, September 12, 2013 at 1:25am by Al

chemistry
Volume (mL) of 2.15 M potassium hydroxide that contains 8.09 g of solute WebAssign will check your answer for the correct number of significant figures. mL
Sunday, October 6, 2013 at 12:26am by john

math
let the amount of 10% solution be x ml then the amount of 15% solution must be 100-x ml .10x + .15(100-x) = .12(100) 10x + 15(100-x) = 12(100) 10x + 1500 - 15x = 1200 -5x = -300 x = 60
Thursday, May 6, 2010 at 7:58pm by Reiny

chemistry
It's just plug and chug. mL x M = mL x M mL x 16M = 5,000 mL x 0.1 M Solve for mL HNO3.
Sunday, February 13, 2011 at 9:13am by DrBob222

chemistry
Use mL x M = mL x M 20 mL x 13M = mL x 0.560 mL will be the final volume needed.
Friday, April 22, 2011 at 7:42pm by DrBob222

biochemistry
0.565 mL/g x 8.0g = ? mL. 35 mL + ?ml = ? mL total volume. Check my thinking.
Thursday, August 30, 2012 at 1:53pm by DrBob222

Chemistry
First determine where the equivalence point is so you will know where you are on the titration curve with each of thes additions. mL x M = mL x M 25.0 x 0.05 = mL x 0.063 mL = about 19 or so. Therefore, 10 mL will be before the e.p. and you will have some base and some of its ...
Sunday, November 11, 2012 at 6:29am by DrBob222

chemistry
500 mL doesn't mean anything without the density. 15% w/w means 15 g H2SO4/100 GRAMS soln. So in 500 GRAMS of soln there is 15 g H2SO4 x 500/100 = ? but in 500 mL who knows.
Tuesday, November 27, 2012 at 6:16pm by DrBob222

science
You add 12.5 mL of 4.15 acetic acid to 25.0 mL of 1.00 M NaOH. Calculate the hydronium ion concentration and pH of the resulting solution.
Monday, March 7, 2011 at 5:45pm by Bill

Chemistry
when 10.0 ml of a .20 M Cu (NO3)2 solution is mixed with 15.0 mL of 0.20M NaOH, what is the theoretical yield (grams) of copper (II) hydroxide?
Wednesday, September 12, 2012 at 7:17pm by Lily

chemistry
What volume in ml of 0.0985 m NaOH solution is required to reach the end point in the complete titration of a 15.0 ml sample of 0.124 M phosphoric acid?
Monday, July 22, 2013 at 11:01am by AmyN

Chemistry
Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added. a)0.0 mL b)20.0 mL c)25.0 mL d)40.0 mL e)50.0 mL f)100.0 mL
Saturday, March 23, 2013 at 4:37pm by Jeff

Chemistry
A 30 mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30 mL, 35 mL, 36 mL, 37 mL, and 40 mL.
Tuesday, March 8, 2011 at 11:43pm by Melissa

Chemistry
A 30 mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30 mL, 35 mL, 36 mL, 37 mL, and 40 mL.
Tuesday, March 8, 2011 at 11:49pm by Melissa

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
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

MATH
A pharmacist mixed some 10%-saline solution with some 15%-saline solution to obtain 100 mL of a 12%-saline solution. How much of the 10%-saline solution did the pharmacist use in the mixture? A 60 mL B 45 mL C 40 mL D 25 mL CAN SOME GIVE AN EQUATION TO HELP MY SOLVE THIS ...
Friday, May 7, 2010 at 8:05pm by Anonymous

CHEM, please help!
A 11 mL sample of a solution of AlBr3 was diluted with water to 23 mL. A 15 mL sample of the dilute solution was found to contain 0.045 moles of Br-. What was the concentration of AlBr3 in the original undiluted solution? answer is 2.09 but i cant get it.
Thursday, February 16, 2012 at 11:07pm by Kate

chemistry
Okay let me write it this way. I mixed 30 mL of 0.1 M Acetic Acid and 15 mL of 0.1 M Sodium Hydroxide and measured the pH. Then I added 5 mL of 0.1 M NaOH to this buffer and measured the pH. It's asking me: Show the calculations for the pH of the buffer before and after the ...
Saturday, July 14, 2012 at 6:28pm by fenerbahce

chemistry
Okay let me write it this way. I mixed 30 mL of 0.1 M Acetic Acid and 15 mL of 0.1 M Sodium Hydroxide and measured the pH. Then I added 5 mL of 0.1 M NaOH to this buffer and measured the pH. It's asking me: Show the calculations for the pH of the buffer before and after the ...
Saturday, July 14, 2012 at 7:42pm by fenerbahce

science
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0 mL of 0.079 M NaOH. Next, you add 1.00 mL of 7.15 10-6 M lidocaine to this mixture Denoting lidocaine as L, calculate the fraction of lidocaine present in the form LH
Sunday, October 6, 2013 at 7:04pm by nick

chemistry
What volume in mL of 0.0985 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 15 mL sample of 0.124 M phosphoric acid?
Sunday, December 9, 2012 at 9:39pm by What?

chemistry
What volume in mL of 0.0985 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 15 mL sample of 0.124 M phosphoric acid?
Monday, December 10, 2012 at 8:06pm by What?

Chemistry-need help ASAP
15 ml of 3.0 M NaOH are added to the following: 500.0 ml of pure water 500.0 ml of 0.1 M formic acid 500.0 ml of 0.1 M formate of potassium 500.0 ml of a solution containing 0.1 M formic acid and 0.1 M formate of potassium. Calculate the difference of pH resulting from the ...
Monday, April 14, 2014 at 8:40pm by Sam

Chemistry
Consider the titration of 100.0 mL of 0.260 M propanoic acid (Ka = 1.310−5) with 0.130 M KOH. Calculate the pH of the resulting solution after each of the following volumes of KOH has been added. (Assume that all solutions are at 25C.) (a) 0.0 mL (b) 50.0 mL (c) 100.0 ...
Wednesday, March 13, 2013 at 2:56am by Margaret

Chemistry
2.5 moles of each implies 86.18g/mole*2.5moles=215.5g 215.5 g / .660 g/mL = 326.4 mL 88.15 g/mole * 2.5moles=220.4g 220.4 g / .814 g/mL = 270.7mL
Tuesday, February 3, 2009 at 11:25pm by DAS

math
2*2.5*3 = 15 m^3 7500 mL = 7.5 m^3 so steel volume = 15 -7.5 = 7.5 m^3 ( ridiculously strong tank )
Thursday, November 22, 2012 at 7:44pm by Damon

chemistry
mL x M = mL x M mL x 12.0 = 500 x 3.5 mL = you can do it---about 60 mL or so. The reason I worked it through is to show you what NOT to do. You DON'T use 60 mL of the concd soln (or whatever the number turns out to be) and add 500 mL of water. Instead, you take 60 (or whatever...
Thursday, March 11, 2010 at 11:00pm by DrBob222

Chemistry
Calculate the pH of a 25 mL sample of distilled water after the addition of 1 mL, 2 mL, 3 mL, 4 mL, and 5 mL of NaOH and HCL. (0.1 M HCl and NaOH) In total, you need to show 10 calculations.
Monday, March 14, 2011 at 9:32pm by Mariah

chemistry
What volume of WATER MUST BE ADDED to 10.0 mL of 6.0 M NaOH to make a solution that is 0.30 M in NaOH? Assume that the volumes are additive. a. 10 mL b. 190 mL c. 200 mL d. 210 mL e. 500 mL
Monday, March 29, 2010 at 6:30am by lawrence

college chem
Calculate the pH of a 25 mL sample of distilled water after the addition of 1 mL, 2 mL, 3 mL, 4 mL, and 5 mL of NaOH and HCL. (0.1 M HCl and NaOH) In total, you need to show 10 calculations.
Monday, March 14, 2011 at 9:50pm by Mariah

chemistry
No. Isn't the first column mL NaOH and the second column is pH. Then between pH 6.5 and 11.2 or so is the vertical portion of the pH and that occurs about 12 mL or so if I read your numbers correctly. A pH of 12 is at 15.0 mL and the curve in that region is almost horizontal.
Saturday, April 5, 2008 at 5:22pm by DBob222

Chem
I have a problem, the density of the metal = mass (2) - mass (1) over Volume (2) - Volume (1) = My first mass and volume are 15.098g and 5.5 mL. the second mass and volume are 11.3235g and 4.0 mL. I got 9.04g/mL as my answer if this isnt right can you walk me through the steps?
Monday, September 27, 2010 at 8:59pm by Jackson

Chemistry
help...If exactly 5.0 mL of HNO3 will neutralize 15 mL of 2.0 M NaOH, what is the molarity of the HNO3 solution? Have no idea what to do. thank you.
Sunday, March 25, 2012 at 9:34pm by Brad

chemistry
Calculate the pH of a solution prepared by mixing 25.0 mL of 0.60 M HC2H3O2 and 15.0 mL of 0.60 M NaC2H3O2?
Thursday, May 6, 2010 at 3:57pm by Julie

chemistry
Calculate the pH of a solution prepared by mixing 25.0 mL of 0.60 M HC2H3O2 and 15.0 mL of 0.60 M NaOH?
Thursday, May 6, 2010 at 3:58pm by Julie

chemistry
How much of a 0.25 M NaOH solution is needed to neutralize 100 mL of a 0.15 M HCl solution? The units are mL
Sunday, October 3, 2010 at 11:53pm by jazmin

Chemistry
15 mL of 60oC water is mixed with 10 mL of 0oC water in a perfect calorimeter. What is the final temperature?
Wednesday, November 2, 2011 at 10:07pm by Paul

pharmacy math
if 500 ml of a 15% solution is diluted to 1500 ml, how would you label the final strength of the solution?
Friday, December 7, 2012 at 1:37pm by cleondra

math
If an IV drop has 15 parts per 1,000 ml, how many parts would there be in 430 ml?
Sunday, February 9, 2014 at 8:30pm by Anonymous

chemistry
15.00 ml of NaOH is obtained in an Erlenmeyer flask. Before titrating with .2500 M HCl, the initial volume of acid in a buret is read as 2.08 ml. At the endpoint the final volume of acid in the buret is 25.20 ml. What was the concentration of NaOH?
Wednesday, November 28, 2012 at 7:32am by lisa

Chemistry
what would be the molarity of a KOH solution if 15 mL of the solution required 22.3 mL of 0.085 M HCl to react with the base?
Tuesday, March 15, 2011 at 9:01pm by Anonymous

chemistry
mL x M = mL x M. 1000 mL x 6M = mL x 3M mL = (1000 x 6)/3 = 2000 mL. Therefore, add 1000 mL
Thursday, April 29, 2010 at 7:10am by DrBob222

chemistry
Which one of the following represents the theoretical yield, in moles, of precipitate for the double displacement reaction if 25.0 mL of 1.0 M aqueous calcium nitrate is added to 15.0 mL of 1.5 M sodium phosphate?
Friday, October 23, 2009 at 7:15pm by Anonymous

Chemistry
Consider the titration of 41.5 mL of 0.213 M HCl with 0.123 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. (Assume that all solutions are at 25C.) (a) 0.0 mL (b) 10.0 mL (c) 40.0 mL (d) 80.0 mL (e) 100.0 mL
Wednesday, March 13, 2013 at 2:55am by Margaret

chemistry Molarity
mL x M = mL x M Substitute and solve for mL. 353 x 1.25 = mL x 0.5 Solve for mL and this will be the FINAL VOLUME. To find how much water must be added requires a. That we assume the volumes are additive. b. Then final volume in mL - 353 mL = mL to be added.
Saturday, December 11, 2010 at 2:17pm 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
15 ml of 0.5 M of HCl is added to a 100 ml sample of 0.2 M HNO2 (Ka for HNO2= 4.0 x 10^(-4)). What is the equilibrium concentration of NO2- ions?
Sunday, April 10, 2011 at 8:21pm by GK

Chem
Calculate the pH of a solution obtained by mixing 50 mL of 0.75 M CH3COOH with 15 mL of 1.6 M NaOH. (Ka of CH3COOH is 1.8 x 10-5)
Thursday, January 23, 2014 at 2:12am by Jamie

chemistry
Consider the titration of 88.0 mL of 0.150 M Ba(OH)2 by 0.600 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 0.0 ml 12 ml 31 ml 44 ml 88 ml
Monday, March 28, 2011 at 1:19pm by Sarah

Math
15 mL in 1 tablespoon 15 * 10 = ?
Monday, April 1, 2013 at 8:03pm by Ms. Sue

Chemistry(reposts #1)
A solution is prepared by dissolving 5.00 g of stannic nitrate in enough water to make 250.0 mL of stock solution. A 15.0 mL aliquot (portion) of this stock solution is then removed and added to 75.0 mL of water. Calculate the concentrations of all ions in the final solution.
Friday, October 25, 2013 at 8:18pm by Anonymous

chemistry
First, decide upon how many mL of the diluted solution you want to make; say 1000 mL, then mL x M = mL x M 1000 mL x 1 M = mL x 17.6 M Solve for mL on the right. So you would take that many mL of the 17.6 M stuff and add water to the mark in a 1 L volumetric flask. Said ...
Monday, February 8, 2010 at 1:13am by DrBob222

osu
a 50.0 ml sample of a 15% (m/v) solution of H2SO4 is added to water to give a final volume of 250.0 ml. What would the final concentration be?
Tuesday, November 23, 2010 at 12:26pm by Kat

Chemistry
If you add enough water to 175.0 mL of a .15 M NaCl solution until the final volume is 350.0 mL, what will the molarity of the diluted solution be?
Tuesday, March 12, 2013 at 7:25pm by Tim

11th grade ..CHEMISTRY
This is a Quantitative Redox titration. (KMnO4) = 1.8 G.. 500 ML after the experiment we had to record the data of the 3 trials. 1. Trial - VolUme FeSO4 = 10.00 Ml - VOlume KMnO4 11.00 Ml 2. Trial - VolUme FeSO4 = 10.00 ML - VOlume KMnO4 11.15 Ml and we ran outa the solution...
Wednesday, November 5, 2008 at 5:16pm by Komal

science
amount= 240*15 micrograms notice units micrograms/ml * ml
Thursday, April 29, 2010 at 10:52pm by bobpursley

Chemistry
For each electron in a ground-state Be atom, select the set of quantum numbers that represents it. Check all that apply. n=1 l=0 ml=-1 ms= +1/2 n=1 l=0 ml=0 ms=-1/2 n=2 l=1 ml=0 ms= -1/2 n=1 l=0 ml=0 ms=+1/2 n=2 l=1 ml=1 ms=+1/2 n=2 1=0 ml=0 ms=+1/2 n=2 l=0 ml=0 ms=-1/2 n=2 l=...
Sunday, March 24, 2013 at 11:39pm by Anonymous

Chemistry
For each electron in a ground-state Be atom, select the set of quantum numbers that represents it. Check all that apply. n=1 l=0 ml=-1 ms= +1/2 n=1 l=0 ml=0 ms=-1/2 n=2 l=1 ml=0 ms= -1/2 n=1 l=0 ml=0 ms=+1/2 n=2 l=1 ml=1 ms=+1/2 n=2 1=0 ml=0 ms=+1/2 n=2 l=0 ml=0 ms=-1/2 n=2 l=...
Sunday, March 24, 2013 at 11:41pm by Anonymous

Chemistry
i have another one i can't get the write answer for... Calculate the pH of the colution that results when 27.38 mL of 0.15 M H2SO4 is mixed with 18.50 mL of 0.19 M Ca(OH)2? Thank you guys so much!!
Sunday, May 22, 2011 at 12:03pm by Laura

chemistry
i have another one i can't get the write answer for... Calculate the pH of the colution that results when 27.38 mL of 0.15 M H2SO4 is mixed with 18.50 mL of 0.19 M Ca(OH)2? Thank you guys so much!!
Monday, May 23, 2011 at 10:35am by Laura

Chemistry
Need help with #2 & # 3 1. Record the pairs of data for pressure (atm) and volume (mL). Pressure(atm) Volume(mL) 1.000 150 mL 1.154 130 mL 1.364 110 mL 1.667 90 mL 2. Does your experimental data verify Boyle's Law? Explain. 3. What pressure would the gas sample have at a ...
Friday, May 14, 2010 at 2:22pm by Ashley

chemistry
The molarity of a solution prepared by dissolving 15.0 grams of NaCl in 100 mL water is 0.15 M. True or False
Monday, December 5, 2011 at 2:20pm by Anonymous

Chemistry
3.10g/ml *1mole Br/79.0g =0.039 mol/ml 0.039mol/ml * 2.00ml =0.0784 mol 1.05 g/ml * 1mol/60g = 0.0175 mol/ml * 125 ml =2.18 mole I dont know where I am going wrong becaus ethe answers are not same????????
Wednesday, February 10, 2010 at 1:32pm by CC

chem
1.15 M NaCl = 1.15 mols/L of solution. How many grams is 1.15 mols? That will be 1.15 mols x molar mass NaCl = approximately 67.3 g/L. How much does the L of solution weigh? It will weigh (has a mass of) 1.07 g/mL x 1000 mL = 1070 g. So our solution is 67.3 g NaCl/1070 g soln...
Wednesday, October 1, 2008 at 10:11pm by DrBob222

college chemistry
What would the [H3O+] be after addition of 5.15 mL of 0.1000 M HCl to 25.00 mL of 0.1000 B (a weak base, Kb = 6.31e-5)?
Thursday, April 3, 2014 at 4:46pm by hershi

chemistry
Calculate the molarity of NaI in a soultion obtained by adding 5.0 mL of 0.2 M NaI to a mixture of 5.0 mL of 0.2 M K2SO4,5.0 mL K2S2O8, 4.0 mL of H2O and 1.0 mL of Starch
Thursday, October 13, 2011 at 7:13pm by krista

Chemistry
c1v1 = c2v2 50*?mL = 0.5 x 500 mL Solve for ?mL. Add ?ml stock to a 500 mL volumetric flask and make to the mark.
Friday, October 12, 2012 at 5:15pm by DrBob222

chemistry
Heres the simplified version: I need to convert Ni to moles: I have a 0.6215 g sample of Ni that was dissolved in 100.00ml of Fe 3+. Then, 15.00 ml of the sample was taken and titrated. It took 26.48 ml of .0200M Cr2072- to titrate the solution. ] I did the following to find ...
Saturday, June 27, 2009 at 2:48pm by dan

Chemistry
You have a solution of 0.15M Ba(OH)2 and a solution of H2SO4 whose concentration you want to determine. You start with 25 ml H2SO4 in the Erlenmeyer and titrate in the Ba(OH)2. At the end of the titration, you find that you have used 20.4 ml Ba(OH)2 and an additional 2.2 ml ...
Wednesday, April 2, 2014 at 6:12pm by Mike Jones

Chemistry
mL x M = mL x M 500 mL x 0.200 M = mL x 12 M solve for mL.
Tuesday, June 8, 2010 at 1:42am by DrBob222

Science
An object weighing 90 N has a volume of 45 mL and a mass of 9.0 g. What is its density? A. 0.10 g/mL B. 0.20 g/mL C. 5.0 g/mL d. 10 g/mL Please and Thank YOU
Tuesday, November 26, 2013 at 11:19pm by Help Scienee

chemistry
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addtion of the following volumes of acid, and plot the pH versus millimeters of HNO3 added. a. 0.00 mL b. 10.2 mL c. 19.9 mL d. 30.0 mL e. 39.8 mL
Monday, June 27, 2011 at 9:02pm by Cindy

chemistry
Which one of the gollowing represents the theoretical yield, in grams, of precipitate for the double displacement reaction if 25.0 mL of 1.75 M aqueous calcium nitrate is added to 15.0 mL of 1.50 M sodium phosphate?
Friday, October 15, 2010 at 2:58pm by Tammy

chemistry
mL x M = mL x M 35.0 mL x 23.0M = mL x 3.00M Solve for mL which will be the TOTAL volume. The volume to be added will be 35.0 mL less than that.
Wednesday, April 13, 2011 at 10:16pm by DrBob222

Chemistry
What is the pH of a solution in which 25 mL of .10 M NaOH is added to 15 mL of .10 M HCl? I have calculated the amount of moles of each, but I'm not really sure where to go from there. Thanks!
Sunday, April 11, 2010 at 11:38pm by Hannah

General Chemistry
A 15.0 ml sample of unknown HCL04 solution requires titration with 25.3 ml of 1.200 M NaOH to reach equivalence point. what is the unknown concentration?
Tuesday, December 14, 2010 at 11:45am by MAX

Chemistry 151
Use the dilution formula for these. c1v1 = c2v2 c = concn v = volume for a. 100 mL x 0.1M = ? mL x 1M Solve for ?mL of the 1M. b. 250 mL x 0.5M = ? mL x 1 M Solve for ?mL of 1 M.
Sunday, March 16, 2014 at 5:18pm by DrBob222

Chem
Plese tell me if these are right. A 15.0-mL sample of NaCl solution has a mass of 15.78g. After the NaCl is evaporated to dryness, the dry salt residue has a mass of 3.26g. Calculate the following concentrations for the NaCl solution. a. %(m/m)= 3.26 x 100 / 15.78 = 20.7 b. %(...
Sunday, November 7, 2010 at 10:48am by Jason

Chemistry
Poor question. What is the FINAL volume. If you assume 20 g sugar in 20 mL solution (which it will not be) or 15 g sugar in 15 mL solution (which it will not be) then convert 20 g sugar to mols.mols = grams/molar mass and M = mols/L soln. Convert 15 g sugar the same way and M...
Thursday, June 20, 2013 at 8:49am by DrBob222

chemistry
You are asked to prepare 150.0 mL of 3.1510−2 M AgNO3. 2.) An aqueous solution is 6.40% methanol CH3OH by mass, with d = 0.988 g/mL} What is the molarity of CH3OHOH} in this solution?
Tuesday, February 16, 2010 at 4:34pm by Andrew

math/nursing
1 kg = 2.2046 lbs. So a 150 pound patient weighs 150/2.2046 kg. = 68 kg. The IV dose is therefore = 1.5 g/kg * 68 kg = 106 g In a 15% solution, volume = 106 g / (0.15 g/ml) = 707 ml.
Friday, June 25, 2010 at 2:18pm by MathMate

chemistry
What's the M of the diluted solution? That will be 5.8M x (45.8/1000) = about 0.26M How many mols in 15.0 g KNO3? That is 15.0/molar mass KNO3 = about 0.15 moles. So what volume of the diluted solution do we need to make 0.15 moles. M = moles/L 0.26 M = 0.15 moles/L L = about ...
Sunday, November 6, 2011 at 1:35am by DrBob222

Instrumental Chem Lab
I didn't plot the data and I can't verify the equation you have for the line; however, just looking at the data suggests that unknown 2 must have a concn of about 7 mg/100 mL [I used 5 mg/100 x (about 15/about 8) = about 9 mg/100 mL) and 10 mg/100 mL x (about 8/about 15) = ...
Saturday, April 16, 2011 at 4:09pm by DrBob222

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