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April 18, 2014

Search: How many mL of .210 M HCl are needed to react completely with 35.0 mL of 0.101M Ba(OH)2

Number of results: 42,290

Chemistry
it would take 30 grams of HCl to react completely with BaCO3, since it's a 1 to 2 ratio 30 grams of HCl = 1 mole/36 grams so it's .83 moles of HCl
Sunday, March 21, 2010 at 12:56pm by Margaret

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

CHEMISTRY
1) An NaOH solution of unknown concentration is titrated with HCl. 51.9 mL of 0.400 mol/L HCl will neutralize 75.0 mL of the NaOH. What is the concentration of the NaOH solution ? Record your answer in decimal notation. I think the answer is 0.277 mol/L. is that right? 2)An ...
Tuesday, January 31, 2012 at 9:17pm by TIANDRA

Chemistry
a. Convert 1.00 g Fe(OH)3 to mols. mols = grams/molar mass. Use the coefficients in the balanced equation to convert mols Fe(OH)3 to mols H^+. mols HCl = M x L. You know mols HCl and M HCl, solve for L and convert to mL. b. M Fe^3+ = mols/L soln You know mols from part a, L ...
Sunday, November 11, 2012 at 5:16pm by DrBob222

chemsitry
I usually do too much work to do these dilution problems but I go about it this way. The first one. 1000 ug/mL x 100 mL = 100,000 ug in the 100 mL flask. We want 30 ug/mL x 50 mL = 1500 ug in the 50 mL flask. (100,000/100 mL) x ? = 1500 and ? = 1500 x 100/100,000 = 1.5 mL. To ...
Sunday, January 31, 2010 at 12:10pm by DrBob222

chemistry
mL x M = mL x M 50.0 x 0.250M = mL x 1.00M Solve for mL.
Wednesday, May 25, 2011 at 4:54pm by DrBob222

Chemistry
The flask shown contains 10.0 mL of HCl and a few drops of phenolphthaein indicator. The buret contains 0.270 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
Monday, November 22, 2010 at 7:02pm by Jason

Chemistry
Calculate the mass of baking soda, NaHCO3, needed to neutralize 3.0 mL of 3.0 M hydrochloric acid, HCl(aq). Ok, so I'm super confused. I have the equation, but I'm stuck with what to do with it. Equation: NaHCO3 + HCL --> NaCl + H2O + CO2
Wednesday, February 27, 2013 at 9:34pm by Sarah

Chemistry
The flask here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains .270 M NaOH. What volume of NaOH is needed to reach the end point of titration? What was the initial concentration of HCl?
Friday, October 4, 2013 at 11:19pm by Chelsea

chemistry
if 125 ml of H2O is added to 50 ml of 0.35 M NaCl, what is the molarity of the resulting solution?
Tuesday, October 19, 2010 at 12:46am by Dana

Chemistry
What is the pH when 25 mL of .20 M CH3COOH has been titrated with 35 mL of .10 M NaOH?
Monday, November 29, 2010 at 8:38pm by Louis

lab
0.4 * 35.5 ml = 14.2 ml.
Sunday, October 24, 2010 at 6:33pm by Henry

CHEMISTRY! DR.BOB PLEASE HELP
Tungsten trioxide (WO3) has a rich yellow color and is often used as a pigment in ceramics and paints. In order to test a ceramic vase for its WO3 content, a 10.19 g sample of the vase was ground and reduced with Pb(Hg) to convert any WO3 to W3 . The resulting W3 was ...
Wednesday, May 29, 2013 at 2:09am by Decisice 2

chemistry dilution
Add 6.67 x 10^1 mL of solvent to 1mL of stock. Converting everything to ug/mL, 200/3 =6.67 x 10^5 uL or 6.67 x 10^1 mL 200ug/(6.67 x 10^5 mL +1 mL)= 2.96ug/mL
Wednesday, February 27, 2013 at 8:54pm by Devron

Math
A doctor needs to administer 2 mL of a 100 mg/mL solution to a 200 pound patient. However, the doctor has the solution available only in 20 mg/mL strength. What volume of the 20 mg/ml solution would be needed to administer the desired dose ?
Monday, July 21, 2008 at 8:48pm by nicole

math
A doctor needs to administer 2 mL of a 100 mg/mL solution to a 200-pound patient. However, the doctor has the solution available only in 20 mg/mL strength. What volume of the 20 mg/mL solution would be needed to administer the desired dose?
Sunday, January 1, 2012 at 12:20am by Jamie

chemistry
I have no idea. You didn't give a mass of AgNO3 used. I can give you a template to use, however, if we assume the mass AgNO3 used initially was 1 gram. Then the original concn was 1 g/10 mL = 0.1 g/mL. Then you took 3 mL of that and diluted to 1000 mL so the new concn is 0.1 g...
Monday, October 5, 2009 at 3:47pm by DrBob222

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

Math
let's try this again... A doctor needs to administer 2 mL of a 100 mg/mL solution to a 200 pound patient. However, the doctor has the solution available only in 20 mg/mL strength. What volume of the 20 mg/ml solution would be needed to administer the desired dose ?
Monday, July 21, 2008 at 8:48pm by LYNN

mastering chemistry
A solution of volume 80.0 mL contains 16.0 mmol HCHO2 and 9.00 mmol NaCHO2. If 1.00 ml of 12 M HCl is added to this, what will be the resulting pH? (the only problem im having for this question is how to approach it, i know that by adding HCl the concentration of the CB would ...
Saturday, February 28, 2009 at 10:43pm by chma11 student

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
Assignment  Calculate the pH, pOH, [H+], and [OH] for each of the following solutions. Show all work. (10 Points) Solution Composition of Starting Materials 1 0.10 M acetic acid 2. 5 mL 0.10 M acetic acid + 5 mL wa 3 1 mL 0.10 M acetic acid + 99 mL water 4 5 mL...
Monday, October 11, 2010 at 12:24pm by Brian

Chemistry
mols Na2CO3 = grams/molar mass mols HCl = 2x mols Na2CO3 (from the coefficients). M HCl = mols HC/L HCl. You know M HCl and mols HCl, solve for L and convert to mL. By the way, you don't need to assume that 3M HCl contains 3 mols HCl/L soln. Why? Because that IS the definition...
Monday, April 30, 2012 at 2:07pm by DrBob222

chemistry
The question as posed makes little sense in terms of significant figures and practicalities. You would not use glassware of 500.00 ml +/- 0.01 ml (5 sig figs) to prepare a solution of 0.25 M (2 sig figs). Incidently a standard 500 ml class A volumetric glassware has an ...
Monday, October 4, 2010 at 1:39am by Dr Russ

Chemistry -- to Dr.Bob
yes, I'll be on tomorrow. If you dilute the acid with 100 mL water, you don't change the mols of acid or the mols of base or the mols of salt formed or the mols of acid remaining. (a) In the NaOH/HCl problem, the only thing that changes is the final mols/L (mols is the same ...
Friday, May 2, 2008 at 9:41pm by DrBob222

Math
3 tbsp =3*15 ml = 45 ml. 250 ml base Total volume = 250+45 ml = 295 ml. Concentration =45 ml / 295 ml = 15% approx. (note: 1 tsp=5ml, 1 tbsp=15ml)
Sunday, August 19, 2012 at 1:46am by MathMate

Chemistry
165 mL x 0.360M = about 59.4 millimols base and 59.4 mmols acid. ..........base + HCl ==> acid I........59.4.....0......59.4 add...............x............... C........-x.....-x........+x E.......59.4-x....0......59.4+x pH = pKa + log (base)/(acid) Look up the pKa for ...
Sunday, November 17, 2013 at 7:47pm by DrBob222

Chemistry
I don't know how to set up this problem...can you help? How many milliliters of 6.00M HCl are required to react with 150 mL of 1.48 M Al(OH)3? Al(OH)3+3HCl to AlCl3 + 3H2O
Wednesday, October 5, 2011 at 11:25am by Nicole

chemistry
A solution is prepared by adding 50 mL of .050 M HCL to 150 mL of .10 M HNO3. Calculate the concentrations. I know I need to find the [H+] and [OH-] but im not sure how.
Sunday, March 7, 2010 at 4:17pm by Dannie

Biochemistry
Which of the following is the correct pH of a 211.7 mL solution (final volume) of pure water after 52.3 mL of 1.00 mM HCl was added?
Tuesday, September 17, 2013 at 11:59pm by Rich

chemistry
What volume of 1.00 M NaOH would be required to neutralize 77.4 mL of 5.4 M HCl? Round to two places after the decimal point and keep it in mL
Thursday, February 20, 2014 at 8:47pm by Corso

chemistry
What volume of 4.50M HCl can be made by mixing 5.65M HCl with 250 mL of 3.55M HCl?
Saturday, July 24, 2010 at 1:25am by casey

chemistry
Concentrated HCL acid is 38% by weight of HCL and has a density of 1.19 g/ml. What is the morality of HCL?
Sunday, September 25, 2011 at 1:48pm by Anonymous

AP Chemistry
What volume of 0.596M K3PO4 is required to react with 29 mL of 0.864 M MgCl2 according to the equation 2K3PO4 + 3MgCl2 -> Mg3(PO4)2 + 6KCl Answer in units of mL
Sunday, October 21, 2012 at 6:51pm by Tara

Analytical chemistry
What is a pH of 20 mL of 0.08 M NH3 added to 40 mL of 0.04 M HCl? NH3 + HCl = NH4+ + Cl- c(NH3)=(0.02L * 0.08M)/0.06L= 0.02667 M c(HCl)=(0.04L * 0.04M)/0.06L= 0.02667 M c(NH4+)=c(HCl) Kb=[NH4+][OH-]/[NH3] Kb=1.76*10^(-5) So i tried to calculate it like this: Kb=[OH-] pOH=4....
Monday, September 2, 2013 at 8:11am by Gloria

AP chem
Consider the titration of 50.00 ml .250 M HBr with .100 M Ba(OH)2. What is the pH after the following additions of Ba(OH)2 to the 50 ml of hydrobromic acid? 0 ml. 15 ml. 25 ml. 50ml. 51ml.
Wednesday, February 5, 2014 at 11:04pm by Dan

chemistry
Suppose the following: HO-C(H2)-C(H2)-OH + 2 HI --> I-C(H2)-C(H2)-I + water How many mL of the first compound* are needed to react with 9.3 grams of HI? (The density of the first compound is A = 1.11 g/mL) *by first compound, i mean HO-C(H2)-C(H2)-OH
Friday, September 2, 2011 at 8:12pm by kc

chemistry
Ka is not needed. mL x M = mL x M.
Sunday, December 5, 2010 at 1:07pm by DrBob222

chemistry
how many mL of 1M HCL is used to make: 100mL of 0.1M hcl 250Ml OF 0.5M hcl 10Ml OF 0.01m hcl
Saturday, March 29, 2014 at 12:21am by Tammy

Chemisty
The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.270 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
Monday, January 14, 2013 at 7:58pm by Paul

Chemisty
The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.270 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
Monday, January 14, 2013 at 7:59pm by Paul

Chemisty
The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.270 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
Monday, January 14, 2013 at 5:11pm by Paul

science
a solution made from 35 mL of ethanol and 65 mL of water produces by what percent concentration of volume
Wednesday, September 26, 2012 at 9:50am by frances

Chemistry
In a titration of 35.00 mL of 0.737 M S, __________ mL of a 0.827 M KOH solution is required for neutralization.
Friday, October 5, 2012 at 5:14am by Charlie

Chemistry
In a titration of 35.00 mL of 0.737 M S, __________ mL of a 0.827 M KOH solution is required for neutralization.
Friday, October 5, 2012 at 5:19am by Charlie

Chemistry
The method looks ok. NaOH + HCl ==> NaCl + HOH mols NaOH = L x M = (1.30 mL/1000) x0.10 = 0.00013 mols HCl = L x M = (8/1000) x 0.10 = 0.0008 Reagent in excess is HCl. Therefore, all of the NaOH will be used, 0.00013 mols NaCl and HOH formed. Mols HCl remaining unreacted is...
Sunday, May 4, 2008 at 3:02am by DrBob222

chemistry
First you want to calculate the (HCl). That's density x 1000 mL x (%/100) x 1/molar mass = M 1.179 x 1000 x 0.36 x (1/36.5) =11.6 M Then c1v1 = c2v2 What H^+ do you want for pH = 1.8? That is 1.8 = -log(H^+) = about 0.0158 c = concn v = volume 11.6 x v = 0.0158 x 4,700 mL v...
Wednesday, February 13, 2013 at 8:30am by DrBob222

chemistry
1.) How much ethanol, C2H5OH, in liters (d=0.789g/ml) must be dissolved in water to produce 190.5 of 1.65 M C2H5OH? (Molarity problem.) 2.) How much concentrated hydrochloric acid solution (36.0% HCl by mass, d = 1.18g/mL}), in milliliters, is required to produce 11.0 L of 0....
Friday, February 12, 2010 at 8:22pm by joe

Chemistry
What is the molarity of 550.0 mL of KOH solution, that reacts completely with 675 mL of a 0.450 M CrCl3 solution?
Monday, September 27, 2010 at 7:28pm by Tara

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

Chemistry
mass of 1000 mL is 1.19 g/cc x 1000 cc = ??g,]. How much of that is HCl? ??g x 0.35 = xx g. How many moles is that? xx g HCl/molar mass HCl. moles/L is definition of molarity.
Tuesday, January 25, 2011 at 2:06am by DrBob222

chemistry
During an experiment, a student adds 1.23 g of CaO to 200.0 mL of 0.500 M HCl. The student observes a temperature increase of 5.10 C. Assuming the solution\'s final volume is 200.0 mL, the density if 1.00 g/mL, and the heat capacity is 4.184 J/(gC), calculate the heat of ...
Wednesday, June 26, 2013 at 12:32am by imstupid

Chemsitry
During an experiment, a student adds 1.23 g of CaO to 200.0 mL of 0.500 M HCl. The student observes a temperature increase of 5.10 C. Assuming the solution\'s final volume is 200.0 mL, the density if 1.00 g/mL, and the heat capacity is 4.184 J/(gC), calculate the heat of ...
Wednesday, June 26, 2013 at 12:33am by imstupid

General Chemistry
200 mL x 0.1M H2PO4^- = 20 millimols. ?mL x 0.5M NaOH =? ........H2PO4^- + OH^- ==> HPO4^- + H2O I.......20........0..........0........0 add...............x................... C.......-x.......-x...........x E.......20-x......0...........x pH = pK2 + log(base)/(acid) ...
Thursday, January 31, 2013 at 11:05am by DrBob222

Chemistry
The minimum amount will be the amount ethanol needed to dissolve 8.0 g at 100 C. That will be 100 mL x (8/5) = 160 mL ethanol needed. How much is lost. 0.4g x (160/100) = solubility of A in 160 mL ethanol at zero C.
Thursday, September 20, 2012 at 7:37pm by DrBob222

chemistry
Please help again. How many grams of lithium are required to completely react with 70.7 mL of N2 gas at STP when given the following reaction: 6Li + N2 = 2Li3N
Saturday, December 3, 2011 at 10:12pm by Lisa

corrected repost chemistry
molar mass CuCl2 = 134.45 8.00M x 0.125L = 1.00 mole CuCl2 in 125 mL. This is 134.45g/125 mL = 1.0756 g/mL in hand. We want 5.9g/50 mL or 0.118 g/mL. We want to dilute by a factor of 1.0756/0.118 = 9.11625 (I know that's too many significant figures). Then 9.11525 x 125 mL = ...
Sunday, November 6, 2011 at 8:39pm by DrBob222

Chemistry
You don't have all of the needed information (e.g., 25 mL of what M HCl?). It would help if you rephrased the question to clearly show what you want.
Tuesday, November 20, 2012 at 9:46am by DrBob222

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

Honors Chemistry
M = mols/L a. If some solvent (L) has evaporated then L is a smaller number and M goes up and it is more concentrated. b. new concn = I would use 0.500M x (35/20) = ? BUT YOU may prefer to use the dilution formula. c1v1 = c2v2 c = concentration v = volume 35 mL x 0.500 = 20 mL...
Friday, May 4, 2012 at 1:13am by DrBob222

chemistry
0.475 g aspirin x 0.682 = g ASA. That amount was placed in 250 mL beaker so the concn (in grams) = g ASA/250 mL. Perform that division and you have g ASA/mL. Now you dilute it 3:100; therefore, the new concn is g ASA/mL x (3 mL/100 mL) = g ASA/mL in the new solution. If you ...
Monday, January 26, 2009 at 1:27am by DrBob222

Biotechnology
how much NaCl is needed to make 1000 mL of 5 mg/mL solution ? please show steps
Saturday, October 31, 2009 at 2:29pm by tifa

Biotechnology
how much NaCl is needed to make 1000 mL of 5 mg/mL solution ? please show steps
Saturday, October 31, 2009 at 2:29pm by sai

Biotechnology
how much NaCl is needed to make 1000 mL of 5 mg/mL solution ? please show steps
Saturday, October 31, 2009 at 2:29pm by jake

CHEMISTRY
Suppose a student adds 25.00 mL of 1.025 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4969 M NaOH. The titration requires 21.3 mL NaOH to reach the endpoint. How many moles of HCl were neutralized by the NaOH?
Monday, April 22, 2013 at 5:28pm by Sarah

CHEMISTRY
Suppose a student adds 25.00 mL of 1.025 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4969 M NaOH. The titration requires 21.3 mL NaOH to reach the endpoint. How many moles of HCl were neutralized by the ...
Tuesday, April 23, 2013 at 12:40am by Jo

Chemistry
Wilh this form a buffer? 50 mL of .10 M HCl; 35 mL of .150 M NaOH WORK: Moles of HCl= .005 Moles of NaOH= .00525 total litres of solution= .05 + .035= .085 L [HCl]= .005 mol/.085 L = .0588 M [NaOH]= .00525 mol/ .085 L = .0618 M Ka of HCl= 1.3*10^6 pKa= -log(1.3*10^6) = -6.114 ...
Monday, March 22, 2010 at 7:26pm by Vanessa

chemistry
An old bottle of 12.3 M hydrochloric acid has only 33 mL left in it. What is the HCl concentration if enough water is added so that the final volume is 513 mL?
Monday, November 29, 2010 at 5:16am by masin

chemistry
mL x M = mL x M 105 mL x 0.25 M = ??mL x 8 M. So you take ??mL of the 8 M and make it to a total volume of 105. The resulting solution will be 0.25 M.
Monday, January 25, 2010 at 7:10pm by DrBob222

Chemistry I
x= unknown mass of H2O x(4.184)(23.5-35) + 17.008(4.184)(23.5-18.2)=0 I don't think so. Tf = final T; Ti = initial T. a. Isn't the initial T 18.2 and not 35 for the unknown amount of water? b. Where did the 17.008 come from? That must be the mass of water but that was 24.4 mL ...
Sunday, October 12, 2008 at 6:16pm by DrBob222

Chemistry
2.00 g = 2.00/molar mass NaOH = about 0.05 moles NaOH and that will take 0.05 moles HCl. mL12M x M12M = mL0.1M x M0.1M mL x 12 = 500 x 0.1 mL of 12M acid = (500 x 0.1/12) = 4.167. I would use a 5.000 mL buret, add exactly 4.167 mL of the 12M stock solution of HCl to the 500 mL...
Friday, November 25, 2011 at 10:11pm by DrBob222

chemistry
Hi, I've watched a tutor solve a simple dilution solutions problem on video. There's a calculation in that problem I wish you could clarify for me. It goes like this: Approximately what volume of water is needed to dilute 25.0 mL of 18.0 M sulfuric acid to 3.0 M ? M * L = M * ...
Saturday, December 11, 2010 at 8:29pm by Cliff

Chemistry
If that is 21.6%(v/v), it means 21.6 mL EtOH/100 mL soln; therefore, 20 mL will contain 21.6 mL EtOH x (20 mL/100 mL) = ?? mL EtOH. Then mass = volume x density.
Saturday, July 24, 2010 at 12:24am by DrBob222

Chemistry
Close but no cigar. 6 mL x 0.05 = xmL*0.02 x mL = 15.0 mL which is the final volume. Therefore, you must add 9 mL to the 6 to make 15.0. Technically, you want the final volume to be 15.0 mL; the amount you add may NOT be EXACTLY 9.0 mL since volumes are not additive.
Thursday, April 18, 2013 at 10:53pm by DrBob222

science
Which of the following samples will react completely with 20.0 mL of 0.200 M LiOH 10.0ML of 0.100 M HCL 10.0mL of 0.200 M H2SO4 10.0mL of 0.100 M HNO3 20.0mL of 0.200 M H3PO4 20.0mL of 0.100 M HBr How do I do this problem??
Saturday, September 26, 2009 at 10:40am by Nisha

chemistry
RATE = ([ Na2S2O3]/time) = k [I-]a [BrO3-]b [HCl]c 1A) You mix together in the proper manner the following: 10.0 mL of .0100 M Potassium Iodide 10.0 mL of .00100 M Sodium thiosulfate 10.0 mL of water 10.0 mL of .0400 M Potassium Bromate 10.0 mL of .100 M HCl The time to turn ...
Wednesday, July 20, 2011 at 9:35pm by Krisha

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
mL NaOH x M NaOH = mL HCl x M HCl
Thursday, March 28, 2013 at 2:24am by DrBob222

chemistry
mL NaOH x M NaOH = mL HCl x M HCl
Wednesday, November 9, 2011 at 4:32pm by DrBob222

chemistry
mL NaOH x M NaOH = mL HCl x M HCl
Friday, November 11, 2011 at 12:52am by DrBob222

chemistry
mL HCl x M HCl = mL NaOH x M NaOH
Thursday, February 23, 2012 at 3:51pm by DrBob222

chem
mL HCl x M HCl = mL NaOH x M NaOH
Wednesday, March 28, 2012 at 9:48pm by DrBob222

percentage
Start with 780 mL milk. Placed 221 mL in glass + 130 mL in cup = 351 mL removed from the jug. How much is left in the jug? That will be 780 mL - 351 mL = 429 % remaining = (429/780)*100 = ?
Saturday, February 11, 2012 at 9:16pm by DrBob222

Chemistry
I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 M sodium acetate and immediately measure the pH. Remove the electrode and add 5 ml of 0.1 M HCL to this buffer. Stir the solution and measure the pH. This is my data: Conc.of...
Thursday, July 16, 2009 at 3:36am by Saira

Chem=continued
Can you make up any quantity, then use 175 mL of that solution or must you make up exactly 175 mL. If the former, the procedure I outlined in my previous post will work ok but you will end up using more chemicals than is necessary AND you will have much more solution that is ...
Monday, February 11, 2008 at 3:37am by DrBob222

Chemistry
How much Na is needed to react with H2O to liberate 179 mL H2 gas at STP? Answer in units of g Please help me with what formulas to use and what to do.
Tuesday, January 29, 2013 at 1:05am by Peter

chemistry
The synthesis of urea by Frederich Whler in 1825 began the decline of the idea that "organic" chemicals could only be made by living organisms as part of their biological processes. AgOCN(aq) + NH4Cl(aq) → AgCl(s) + NH2CONH2(aq) If you perform this reaction and collect ...
Sunday, October 16, 2011 at 10:04pm by Anonymous

Chemistry
mols HCl initially = 0.025 x 0.1 = 0.0025 To end up with pH = 3 (0.001M H^+) we want H^+ to be 1E-3. If we work in millimols and let x = mL of 0.1M NaOH, we have then [(25.00 x 0.1M)-(0.1x)/(25+x)] = 1E-3M Solve for x and I obtained approx 24.5 mL of 0.1M NaOH that must be ...
Wednesday, February 26, 2014 at 7:44pm by DrBob222

Chemistry
Sometimes biochemists (I assume you are in a bio class) use funny symbols and nomenclature (at least in my opinion). Here is a web site that will explain some about dilutions. http://www.stolaf.edu/people/muth/Appendix%20II.pdf If I read this correctly, 1:200 means you want 1 ...
Sunday, July 29, 2012 at 1:00pm by DrBob222

chemistry
What is the pH of the solution created by combining 2.20 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)?
Saturday, April 17, 2010 at 7:23pm by bme1

chemistry
What is the pH of the solution created by combining 0.80 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)?
Monday, July 12, 2010 at 4:33am by Cindy

Chemistry
Use the following balanced equation. 3Sr(OH)2 + 2H3PO4 --> 6H20 + Sr3(PO4)2 How many mL of 0.10 M Sr(OH)2 are required to react with 30 mL of 0.30 M H3PO4?
Monday, June 20, 2011 at 4:11pm by Brea

Chemistry
mL x M = mL x M Solve for the M of the diluted HCl, then plug into the pH equation. Then pH = -log(H^+) = ??
Wednesday, April 6, 2011 at 6:14pm by DrBob222

Chemistry
An antacid tablet containing magnesium hydroxide instead of calcium carbonate was dissolved in 100.0 mL of 0.2893 M HCL. 10 mL of this solutions was titrated to endpoint with 25.20 mL of 0.1007 M NaOH. How much magnesium hydroxide was in the antacid tablet(in mg)? Any help is ...
Tuesday, May 7, 2013 at 9:28pm by Mindy

chemistry college
The secret to these is to recognize what you have in the solution at each addition. The first thing you do is to determine where the equivalence point is; i.e., number of mL HCl added to get to the equivalence point. 20 mL--you have a mixture of NH3 and NH4Cl. That makes a ...
Wednesday, December 4, 2013 at 5:33pm by DrBob222

chem lab (webwork)
Complete the table below: How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid? Base Acid Base Volume (mL) NaOH HCl NaOH HC2H3O2
Tuesday, April 13, 2010 at 7:19pm by need help student

Statistics
Total plasma volume is important in determining the required plasma component in blood replacement theory for a person undergoing surgery. Plasma volume is influenced by the overall health and physical activity of an individual. Suppose that sample of 50 male firefighters are ...
Thursday, June 24, 2010 at 5:06pm by stan

chemistry
8 mL of 0.0100 M HCl are added to 22 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?
Friday, October 21, 2011 at 8:40pm by annie

chemistry
Calculate the molarity of a solution prepared by diluting 200.0 mL of 4.0 M HCl to 500.0 mL of solution a. 1.1 M b. 1.6 M c. 2.7 M d. 10. M
Sunday, December 11, 2011 at 4:32pm by anonymous

Chemistry
What is the pH of a solution of 40.0 ml of 0.800 M HCl titrated with 4.00 ml of 1.00 M Hydroxyl amine?
Wednesday, April 24, 2013 at 10:43pm by Sara

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