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April 20, 2014

Search: HCl and NaOH

Number of results: 8,280

chemistry
This may help. ............NaOH + HCl ==> NaCl + H2O initial....0.001..0.009.....0......0 change...-0.001..-0.001....+0.001..0.001 equil.......0.....0.008.....0.001.0.001 The base and acid react. So 0.001 moles NaOH "disappear" and take 0.001 moles HCl with it (to make 0....
Tuesday, November 8, 2011 at 7:12pm by DrBob222

math
50gm of a sample of ca(oh)s is dissolved in 50ml of 0.5N hcl solution. The excess of hcl was titrated with 0.3N -naoh. The volume of naoh used was 20cc. Calculate of naoh used was 20cc. Calculate % purity ca(oh)2 Who help me step by step
Sunday, December 22, 2013 at 12:31pm by Fai

Chemistry 11
the concentration of HCl, a strong acid is 0.500 M. if 20.0 ml HCl is needed to titrate 40.0 ml of NaOH, what is the concentration of NaOH Help me please. I'm confused by this
Thursday, April 26, 2012 at 3:40am by Jessie

Chemistry
1.Mass of Table: 1.2173g 2.Volume of HCl added: 75.0 mL 3.Milliomoles of HCl added:(0.1845M x 75.0mL= 13.84 mmoles 4.Volume of NaOH used: 17.14 mL 5.Millimoles of NaOH used in titration: (0.1482M x 75.0mL= 11.12 mmoles No, mmoles NaOH used is mL NaOH x M NaOH = 17.14 x 0.1482...
Monday, October 18, 2010 at 11:11pm by DrBob222

chemistry
The beaker contains 0.3000 M HCl and the buret contains 0.3000 M NaOH. Write a complete balanced equation for the neutralization reaction between HCl and NaOH.
Sunday, March 27, 2011 at 1:19pm by Kat

Chemistry
NH3 + HCl ==>NH4Cl Excess HCl + NaOH ==> NaCl + H2O Mols HCl added initially = M x L = 0.1M x 0.050L = ? mols NaOH to neutralize excess HCl = M x L = 0.025M x 0.02150 = ? mols HCl used by ammonia = mols initially - mols excess = ? = mols NH3 initially. M NH3 = mols NH3/L...
Sunday, February 2, 2014 at 1:49pm by DrBob222

Chemistry
HCl is an acid. NaOH is a base. general equation is as follows: an acid + a base = salt + water HCl + NaOH ==> NaCl + H2O
Sunday, September 29, 2013 at 12:39pm by DrBob222

Chemistry
First the M of HCl must be determined from the titration with NaOH. NaOH + HCl ==> NaCl + H2O Since the molar ratio or the reactants is 1:1, one may use mL x M = mL x M. Use that to determine M HCl. Then go to the Ca(OH)2 solution. 2HCl + Ba(OH)2 ==> BaCl2 + 2H2O Here ...
Monday, May 3, 2010 at 1:46pm by DrBob222

Chemistry - repost
Why 7ml of 10M HCl? Do I add 7ml of 10M HCl 1st slowly in ice bath, then slowly adjust the pH to 7 using 10M HCl? Then to dilute to 15ml in a graduated cylinder? Thanks Posted by candy on Tuesday, September 21, 2010 at 10:03am. The following is part of a procedure for a limit ...
Tuesday, September 21, 2010 at 3:12pm by candy

Chemistry
CaCO3 + 2HCl ==> CaCl2 + H2O + CO2 1. mols HCl added = 1.5L x 1.45M = about 2 mol HCl but you need to do it more accurately. That reacts with all of the CaCO3 but doesn't use all of the HCl. 2. Excess HCl requires how many mols. That's 0.850L x 0.543M NaOH = about .46 mols ...
Monday, December 3, 2012 at 10:31pm by DrBob222

Grade 12 chemistry
This is the second reaction: HCl(aq)+NaOH(aq)-->NaCl(aq)+H2O(l) (Heat of neutralization) This reaction involves mixing two solutions: 1.00 mol/L NaOH and 1.00 mol/L HCl. Trial 1: 48.0 mL of the NaOH solution is mixed with 47.5 mL of the HCl. The temperature rises from 22.00...
Sunday, January 1, 2012 at 11:08pm by tessa

Chemistry
mols NaOH initially = M x L = ? mols HCl added = M x L = ? mols NaOH remaining = mols NaOH - mols HCl. Then (OH^-) = (NaOH) and pOH = -log(OH^-) Then pH + pOH = pKw = 14. You know pKw and pOH solve for pH.
Wednesday, May 1, 2013 at 12:33am by DrBob222

Chemistry - DrBob222
Alright, I've made a list of reactions that would produce precipatations. NaCl + Zn CaCl2 + NaOH CaCl2 + Zn CaCl2 + Na2SO4 CuSO4 + NaOH CuSO4 + Zn NaOH + AgNO3 NaOH + Zn BaOH2 + AgNO3 BaOH2 + Zn BaOH2 + Na2SO4 So this way I can figure if it is NaCl, CaCl2, CuSO4, NaOH,Ba(OH)2...
Sunday, November 11, 2007 at 8:34pm by Raj

chem
This is too long and too detailed to post; in general what you do is start with mols HCl, add x mols NaOH, subtract mols to see mols HCl unreacted, then M = mols/L (remember this is total volume which is mL HCl to start plus mL NaOH added). Then pH = -log(H^+) I can expand on ...
Wednesday, March 28, 2012 at 10:03pm by DrBob222

Chemistry
I don't know about the end point because I don't know what indicator you are using; however, I can tell you about the equivalence point (you must be careful with those two words.) mols HCl = M x L = ? mols NaOH = mols HCl M HCl = moles HCl/L HCl. You know mols and M, solve for L
Tuesday, March 13, 2012 at 1:02am by DrBob222

chem
NaCN and NaOH HCN and NaOH HCl and NaCN HCl and NaOH
Tuesday, April 12, 2011 at 7:04pm by Anonymous

Chemistry
Sorry DrBob, it's me again! Here's the info: Antacid Brand: Life Concentration of HCl: 0.1845 M Concentration of NaOH: 0.1482 M Trial 1: 1.Mass of Table: 1.2173g 2.Volume of HCl added: 75.0 mL 3.Milliomoles of HCl added:(0.1845M x 75.0mL= 13.84 mmoles 4.Volume of NaOH used: 17...
Monday, October 18, 2010 at 11:11pm by Akhed-To DrBob222

chem.
A clarifying note: The NaOH is a solid and HCl is a gas. They will not react in that state. Most of the time we omit the fact that we use solutions but if we want to do it up brown, we would write HCl(aq) + NaOH(aq) ==> NaCl(aq) + H2O(l) Thanks for using Jiskha.
Friday, December 19, 2008 at 10:10am by DrBob222

Organic Chemistry
For (a) carboxylic acids, I wrote: R-COOH + NaOH --> R-COONa + H20 This is OK. I don't know if its required or not but you can also show the ionization of RCOONa ==> RCOO^- + Na^+. R-COONa + HCl --> R-COOH + NaCl (I'm not sure if I am supposed to give the equation of ...
Saturday, September 27, 2008 at 3:17am by DrBob222

Chemistry - bobpursley pls help
Posted by candy on Tuesday, September 21, 2010 at 3:12pm. Yes, my NaOH is granular. Why 7ml of 10M HCl? Do I add 7ml of 10M HCl 1st slowly in ice bath, then slowly adjust the pH to 7 using 10M HCl? Then to dilute to 15ml in a graduated cylinder? Thanks Posted by candy on ...
Tuesday, September 21, 2010 at 4:47pm by candy

Chemistry
4. A 5.309 g antacid tablet, with CaCO3 as the active ingredient, was mixed was 30.0 mL of 0.831 M HCl. It took 15.3 mL of 0.7034 M NaOH to neutralize the excess acid. a) Calculate the volume of HCl neutralized by the NaOH. b) Calculate the amount of HCl (in mL) neutralized by...
Tuesday, April 2, 2013 at 9:53pm by Josh

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
1.9 mol HCl and 3.8 mol NaOH react according to the equation HCl + NaOH −→ NaCl + H2O . Calculate the amount in moles of NaCl formed. Answer in units of mol
Thursday, February 9, 2012 at 8:33pm by Mary

chemistry
Im stuck on these few questions that seems to be getting me no where : c HCl = 0.1812 c NaOH = 0.1511 volume of HCl added : 75 volume of NaOH added: 29.23,19.58,33.3 -Determine the number of mmoles of HCl that did not react with the anatacid. - mmoles of HCl neutralized by the...
Tuesday, October 8, 2013 at 7:56am by kathy

chemistry
Im stuck on these few questions that seems to be getting me no where : -Determine the number of mmoles of HCl that did not react with the anatacid. c HCl = 0.1812 c NaOH = 0.1511 volume of HCl added : 75 volume of NaOH added: 29.23,19.58,33.3 - mmoles of HCl neutralized by the...
Tuesday, October 8, 2013 at 1:22am by karen

Math
NaOH v= 30mL, M=0.10 HCI v= 25.0 mL, M=? You need exactly the same number of moles (or molecules) of NaOH as of HCl .1 * 30 = M * 25 M of HCl = .1 (30/25) = .12
Monday, March 8, 2010 at 11:11am by Damon

Chemistry
Sorry DrBob, it's me again! Here's the info: Antacid Brand: Life Concentration of HCl: 0.1845 M Concentration of NaOH: 0.1482 M Trial 1: 1.Mass of Table: 1.2173g 2.Volume of HCl added: 75.0 mL 3.Milliomoles of HCl added:(0.1845M x 75.0mL= 13.84 mmoles 4.Volume of NaOH used: 17...
Tuesday, October 19, 2010 at 12:34am by Akhed-To DrBob222

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 DrBob
The NaOH + HCl part you know how to do from the previous problem I worked. And you are right about the volume of base not changing if the solution is diluted AFTER putting it in the titration vessel. For the NaOH + HC2H3O2 problem, you need to write the equation. It is NaOH + ...
Thursday, May 1, 2008 at 4:53pm by DrBob222

CHemistry- For Dr.Bob
Hey Dr.Bob, I asked two days ago a question about a titration lab I had that you answered, but I still have one more question about that lab. Here's the lab summary: For my chemistry of solutions class, we had a titration lab where we titrated NaOH into an HCl + H2O mix. This ...
Thursday, August 2, 2012 at 6:01pm by Robert

Chemistry
construct the balance equation for NaOH and HCl reaction obtain a mole ration i.e. 1:1 determine the actual mole of NaOH reacting using c=n/v where c is 0.1 and v is 54 use this mole to find the concentration of HCl using c=n/v hope that helps
Sunday, May 12, 2013 at 10:39pm by bonjo

math Steve form your help
50gm of a mixture of ca(OH)2 is dissolved in 50ml of 0.5N hcl solution, the excess of hcl was titrated with 0.3N -naoh. The volume of naoh used was 20cc. Calculate % purity of ca(OH)2 The answer 41.35% Who helps me step by step
Sunday, December 29, 2013 at 12:20pm by Fai

CHEMISTRY
is the equation NaOH + HCl-> NaCl + H2O? I do not understand "Subtract the obtain the HCl concn." How do I calculate the HCl concn?
Sunday, October 17, 2010 at 4:50pm by Cindy

chemistry
given the reactant amounts specified in each chemical eguation, determine the limiting reactant in each case: a. HCL+NaOH->NaCl+H2O 2.0 mole of HCl 2.5 mole NaOH b. Zn+2HCl->ZnCl2+H2 2.5 mole Zn 6.o mole HCl c. 2Fe(OH)3+3H2SO4->Fe2(SO4)3+6H2O 4.0 mole Fe(OH)3 6.5 mole...
Wednesday, March 3, 2010 at 6:43pm by christina

Chemistry
If 5.00 mL of HCl require 4.59 mL of 0.9581 M NaOH to just consume the HCl, what is the concentration of the HCl?
Monday, February 22, 2010 at 5:37pm by Caryn

chemistry
If 5.00 mL of HCl require 4.03 mL of 0.9581 M NaOH to just consume the HCl, what is the concentration of the HCl?
Sunday, July 25, 2010 at 2:58pm by Ellen

Chemistry
I posted before about designing a procedure to determine two unknowns (1 solid, 1 solution). The possible solutions were: NaCl, CaCl2, CuSO4, NaOH,Ba(OH)2, HCl, HNO3, or H2O. The reagents given are: NaOH, HCl, AgNO3, Zn metal, Na2SO4, and H2O. The procedure I've designed so ...
Sunday, November 11, 2007 at 5:59pm by Raj

chemistry
There are two problems here. #1. pH when adding 1.90 mL of 0.1 M NaOH to 8.00 mL of 0.1 M HCl. moles NaOH = M x L = 0.0019 x 0.1 = 0.00019 moles moles HCl = 8.00 mL x 0.1 M = 0.008 x 0.1 = 0.0008. NaOH + HCl ==> NaCl + H2O Place the moles below the reactants so you can see ...
Sunday, July 11, 2010 at 8:46pm by DrBob222

chemistry
A student titrated 10.00mL aliquots of her unknown amino acid solution with standard 0.1521M NaOH and with 0.0986M HCl. Inflection points were determined in the graphs after 3.29mL of HCl and 18.61mL of NaOH were added. Calculate the concentration of the amino acid
Thursday, August 5, 2010 at 2:55am by Brandon

Chemistry
Antacid tab is dissolved in water and a few drops of phenolphthalein is added yielding bright pink solution. 0.2025 M HCl added until pink color disappears. The 0.2147 M NaOH added until it turns light pink for ~30 seconds. mass on antacid tablet = 1.056g initial V 0.2025 M ...
Saturday, December 1, 2012 at 4:43pm by T

chemistry
Unless I have really missed something, and I don't think I have, there is no correct answer. There is no unknown to determine. 5.00 mL of 3 M HCl CAN'T require 14.45 mL of 1.00 M NaOH. moles = M x L. For HCl that is 0.005 x 3.00 M = 0.015 moles. NaOH titrated it. 0.01445 x 1....
Sunday, June 13, 2010 at 12:03am by DrBob222

Chemistry
the concentration of HCl, a strong acid is 0.500 M. if 20.0 ml HCl is needed to titrate 40.0 ml of NaOH, what is the concentration of NaOH I don't understand how to do this. Can I see a step by step way of how to do this please
Monday, May 23, 2011 at 5:51pm by Lilly

Chemisty
I posted a response earlier that you don't have enough information to answer this question. There are four items you need. 1. volume HCl 2. M HCl 3. volume NaOH 4. M NaOH. You need any three of the four, then you can calculate the fourth..
Monday, January 14, 2013 at 7:58pm by DrBob222

chemistry
We had a Chemistry lab for buffer system, we used HCl and NAOH. We did a graph ( PH vs ml of HCL and NaOH, we told to estimate the buffer capacity using the graph. How to do this?
Saturday, April 14, 2012 at 11:07am by Mima

chemistry
mols HCl = M x L = ? mols NaOH = M x L = ? Subtract, the one in excess will determine the acidity/basicity. If acid then pH = -log(HCl). If basic then pOH = -log(NaOH), then convert to pH.
Wednesday, May 2, 2012 at 1:46pm by DrBob222

Chemistry
a 15.00mL sample of NaOH was titrated to the stoichiometric point with 17.40mL of 0.2340M HCl. a) what is the molar concentration of the NaOH solution? b)calculate the grams of NaOH in the solution.
Thursday, December 9, 2010 at 9:08am by prince

Chemistry
Hello, I need help with calculations for lab. I prepared excess NaOH and HCL solutions (unknown conc., ~0.1M). Then I standardized my NaOH solution by titrating known amounts of KHP (Potassium hydrogen phthalate)with it in the presence of phenolphthalein (indicator turns pink ...
Sunday, September 20, 2009 at 2:05pm by Pavel

chemistry steps check
Well, I did NOT make an error in my calculations. But I goofed big time. Notice that the NaOH is the excess, not HCl. (There is more NaOH to begin than there is HCl.) Therefore, the 0.00031 is the mol NaOH left unreacted. That means the 1.79 you calculated is the pOH. Just ...
Friday, May 2, 2008 at 11:45pm by DrBob222

CHEM HELPP!!!
Imagine that you are in chemistry lab and need to make 1.00 of a solution with a pH of 2.50. You have in front of you 100 of 7.0010−2 , HCL 100 of 5.0010−2 , and NaOH plenty of distilled water. You start to add HCL to a beaker of water when someone asks you a ...
Tuesday, March 10, 2009 at 3:38am by Ashley

chemistry
A flask containing 5.00mL of 3 M HCl solution requires 14.45mL of 1.00 M NaOH for titration. How many moles of HCl are present in the solution? The density of 3 M HCl is 1.05g/mL
Saturday, June 12, 2010 at 11:12pm by John

chemistry
A flask containing 5.00mL of 3 M HCl solution requires 14.45mL of 1.00 M NaOH for titration. How many moles of HCl are present in the solution? The density of 3 M HCl is 1.05g/mL
Sunday, June 13, 2010 at 12:03am by John

chemistry
25 ml HCl x 1L/1000mL x .200HCl/1L = .005 mol HCl. Using the balanced equation from this, how many moles of NaOh will you need to completely neutralize the HCl?
Wednesday, November 10, 2010 at 11:29am by Zac

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
1)How many milliliters of 1.5 M NaOH will react completely with 448 mL of 0.600 M HCl? NaOH (aq) + HCl (aq) NaCl (aq) + H2O (l) 2)What is the percent yield of the following reaction if 15 g H2O are obtained from the combustion of 18 g C2H6? 2 C2H6 (g) + 7 O2 (g) 4 CO2 (g...
Sunday, October 24, 2010 at 5:24pm by Chicka

organic chemistry
Structures can't be drawn on the boards. But you can easily draw this with pen and paper. Draw the 1-naphthylamine compound and to the Ar-NH2 show with HCl to form Ar-NH3Cl. So this is a salt (this is the hydrochloride of the original amine). With NaOH, just pull the HCl off ...
Thursday, February 5, 2009 at 11:39pm by DrBob222

chemistry
Which of the following mixtures will be a buffer when dissolved in a liter of water? a. 0.1 mol Ca(OH)2 and 0.3 mol HI b. 0.3 mol NaCl and 0.3 mol HCl c. 0.4 mol NH3 and 0.4 mol HCl d. 0.2 mol HBr and 0.1 mol NaOH e. 0.2 mol H3PO4 and 0.1 mol NaOH i think e is answer but not ...
Friday, May 21, 2010 at 6:18am by George2

Chem
Is sodium benzoate soluble in HCl? I put yes What about NaOH? It's supposed to be created from a reaction with benzoic acid and NaOH What about NaHCO3? And aq. sodium benzoate plus HCl? And aq. sodium benzoate plus NaOH?
Tuesday, May 25, 2010 at 8:48pm by Alex

chemistry
Calculate the pH from the addition of 10 mL of a 0.10 M NaOH solution to 90 mL of 0.10 M HCl. okay so i understand how to do most of it but i get messed up at one part.. so i made my equation: NaOH + HCl -> H2O + NaCl (strong base, strong acid= complete dissociation) so net...
Tuesday, November 8, 2011 at 7:12pm by BOB PLEASE HELP!:)

chemistry
moles HCl = moles NaOH moles = M x L moles HCl = 0.1 M x 0.010 L = 0.001 moles. moles NaOH must be 0.001. moles NaOH = M x L; rearrange to L = moles NaOH/M NaOH = 0.001 moles/0.3 = ??
Monday, May 18, 2009 at 11:38am by DrBob222

High School Chemistry
10mL of 0.10M HCl is given. What is the pH? How many milliliters of 0.10M NaOH would be required to neutralize it? What is the pH of the neutralized solution? What would the pH of the solution be if you added 20mL of NaOH? Here's what I have so far: pH of HCl=-log(0.10M)= 1 ...
Monday, March 21, 2011 at 12:58am by Becky

pH- really hard one
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)? NaOH + HCl ==> NaCl + H2O So all the NaOH is neutralized leaving NaCl, which will not affect the pH either way, ...
Sunday, April 15, 2007 at 7:39pm by Christine

Chemistry
determine the approximate molarity of a solution of NaOH prepared by diluting 10ml of 6M NaOH to a volume of 400 ml. using the solution in the first part, 24.5ml of NaOH solution was required to neutralize 26.4ml of a .150M HCl solution. find the molarity of NaOH
Thursday, February 28, 2008 at 10:37pm by Chuck

Chemistry
1. The TOTAL OH should be determined from moles HCl used in the titration. The HCl can't tell the difference between NaOH OH and Ca(OH)2 OH and you obtain total OH with this titration. 2. You know how much OH is there due to NaOH from its concn and volume added. 3. Thus, the ...
Wednesday, April 14, 2010 at 1:49pm by DrBob222

chem
It's a little difficult to read but as I understand it, I think you have failed to take into account the dilution by the water. 1.00 mL x 0.1M NaOH = 0.1 millimols NaOH 8.00 mL x 0.1 M HCl = 0.8 mmols HCl Excess HCl = 0.7 mmol and M HCl = 0.7mmol/101 mL = 0.00693 and pH = ...
Tuesday, May 1, 2012 at 5:20pm by DrBob222

Chemistry
moles HCl = M x L = ?? moles HCl = moles NaOH because the reaction is 1 mole to 1 mole. Write the equation. Then M NaOH = moles/L. Solve for L (and convert to mL if desired.)
Sunday, June 27, 2010 at 5:27pm by DrBob222

Chemistry
I need help I can't seem to get the right answer. Please help! 1/2 H_2 (g) + 1/2 Cl_2 (g) --> HCl (g) -92.3 kJ/mol Na(s) + 1/2 O_2(g) + 1/2H_2(g) --> NaOH(s) -426.8 kJ/mol NaCl(s) --> Na(s) + 1/2Cl_2(g) 411.1 kJ/mol H_2O(l) -->H_2(g) + 1/2O_2(g) 285.8 kJ/mol HCl(g...
Friday, November 8, 2013 at 9:22pm by Alex

Chemistry
mols HCl = M x L = ? mols NaOH = M x L = ? Subtract. Excess mols = either mols HCl or NaOH, then determine OH or H^+ from that.
Friday, May 11, 2012 at 12:39am by DrBob222

chemistry
acid: HCI 0.10 M Base:NaOH O.050 M 3 ml of HCI was used. Calculate the volume of base required to reach the equivalence point of this titration. Somewhere in the finding the solution, i have to use the fact that Moles HCl = moles NaOH. this is what i have so far: Volume of ...
Tuesday, March 3, 2009 at 1:59pm by Anonymous

chemistry- some help plzz totally lost on this one
Start with 100 mL HCl, left with 83.0 means you have added 17.0 mL HCl to the beaker. Start with 100 mL NaOH, left with 88 mL means you have added 12 mL NaOH. Calculate moles HCl and moles NaOH added and subtract to determine the excess acid in the beaker. Then use pH 2.70 to ...
Monday, July 13, 2009 at 1:15pm by DrBob222

Chemistry
The long way but it always works. Write the equation and balance it. HCl + NaOH -->NaCl + H2O moles KOH = M x L = 5M xs 0.002L = ?? Using the coefficients in the balanced equation, convert moles KOH to moles HCl. You can see that the ratio of HCl to KOH is 1:1 in the ...
Wednesday, April 27, 2011 at 10:40pm by DrBob222

science
Hey, holidays is over. Time to get back to work. whats the answer to this one find the concentration of hcl in g hcl/kg Naoh + Hcl---> b +c 2.991 mol 25.00mL Density=0.952g/ml also Hcl=36.46g/mol I got approx 4.58 x 10^3 g/mol of the top of my head
Tuesday, September 1, 2009 at 1:08am by Jim_R

CHEMISTRY
ANTACID TABLET OF WEIGHT 1.3183G WAS DISSOLVED IN 75 MLOF CONC. HCl OF 0.1807M IS TITRATED WITH 20.36ML OF CONC. NaOH OF 0.1481M . FIND MILIMOLES OF HCl ADDED, FIND MILIMOLES OF NaOH USED IN TITRATION, FIND MILIMOLES OF HCl THAT DID NOT REACT WITH ANTACID, FIND MILIMOLES OF ...
Sunday, October 16, 2011 at 7:04pm by Anonymous

Chemistry
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you * 100 mL of 6.0010−2 M HCl, * 100 mL of 5.0010−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone ...
Thursday, July 9, 2009 at 3:16am by Saira

Organic Chemistry
We've been working on extraction of known/unknown compound mixtures lately, and we have to give equations for the acid-base reactions that occurs between HCl, NaOh and (a) R-COOH (b) R-NH2, and (c) Neutral compounds (naphthalene and triphenylmethanol) For (a) carboxylic acids...
Saturday, September 27, 2008 at 3:17am by Jess

GChem
1. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH when 30mL of NaOH have been added? 2. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH after 15mL of NaOH have been added? I don't know how to make calculation I assumed that for number 1 when you have ...
Monday, August 10, 2009 at 12:20pm by Mike

chemistry
I don't think I said that. I said that few people will count strong acids or strong bases as buffers BUT they do show regions where they show buffering action, especially if they are concentrated (for example in 1 or 2 M HCl) titrated with a strong base. For example, if we ...
Thursday, May 12, 2011 at 11:32pm by DrBob222

Chem
What in the world is Tt.That may be "It is found that....". mL HCl x M HCl = mL NaOH x M HCl
Friday, May 3, 2013 at 1:11am by DrBob222

chemistry
Given the thermochemical equation below, calculate the amount of energy released when 250. g of NaOH (molar mass = 40.0 g/mol) reacts with an excess of HCl. Report answer to the correct number of significant figures in units of kilojoules, kJ. NaOH + HCl --> NaCl + H2O ...
Thursday, April 25, 2013 at 9:31pm by sarah

chemistry
Titrating an acid/base - 1 M. solution of NaOH into HCL. I have to Calculate the molarity of the HCl from the volumes of acid and base at the equivalence point and the molarity of the NaOH. This is what I have: Volume of Acid (HCL) at equivalence point: 25ml Volume of Base (...
Wednesday, February 27, 2008 at 4:40pm by Julie

chemistry
Titrating an acid/base - 1 M. solution of NaOH into HCL. I have to Calculate the molarity of the HCl from the volumes of acid and base at the equivalence point and the molarity of the NaOH. This is what I have: Volume of Acid (HCL) at equivalence point: 25ml Volume of Base (...
Wednesday, February 27, 2008 at 4:40pm by Julie

chemistry
Titrating an acid/base - 1 M. solution of NaOH into HCL. I have to Calculate the molarity of the HCl from the volumes of acid and base at the equivalence point and the molarity of the NaOH. This is what I have: Volume of Acid (HCL) at equivalence point: 25ml Volume of Base (...
Wednesday, February 27, 2008 at 4:40pm by Julie

Chemistry
Determine the moles of ammonia in the following cobalt ammine complex: A sample of .1500 g of the cobalt ammine complex is places in a flask and 25.00mL of .200M HCL is added. a few drops of bromocresol green is added and the titration with .100M to NaOH required 16.42mL. I ...
Tuesday, March 16, 2010 at 4:13pm by james

Chemistry
The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated ...
Wednesday, October 20, 2010 at 1:48am by James

College Chemistry
"A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated cylinder to obtain ...
Wednesday, October 20, 2010 at 10:49am by James

chemistry
0.0019L mols of NaOH That was 0.0019 K x 0.1 M = 0.00019 moles NaOH 0.008L x 0.1M HCL = 0.0008 mols HCL 0.00019 - 0.0008 = -0.00061 mols OH left over The larger number is 0.0008 so it will be left over. 0.0008 HCl - 0.00019 NaOH = +0.00061 moles HCl left over. Total Volume: 0....
Sunday, July 11, 2010 at 10:08pm by DrBob222

Chemistry
You can see I made a typo in the post but I corrected it later. mols NaOH = L x M = 0.06705 L x 0.01500 = 0.00100575.This is correct mols HCl = the same thing of 0.0010125 This should read the same thing of 0.00100575. The Molarity HCl = mols HCl/L HCl = 0.00100575/0.025 = 0....
Wednesday, February 20, 2008 at 9:22pm by DrBob222

chemistry
How much HCL would be needed to neutralize 250mL of 6 M NaOH (HCL = 1.5 M)?
Thursday, February 23, 2012 at 3:51pm by Rachel

chemistry
A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after...
Monday, August 6, 2012 at 8:00pm by Anon

chemistry
11.4 mL x 0.1M NaOH = 1.14 mmoles NaOH. 8.00 mL x 0.1M HCl = 0.800 mmoles HCl. 9.00 mL x 0.1M HAc = 0.800 mmoles HAc ...........NaOH + HCl ==> NaCl + H2O initial..1.14....0.800.....0......0 change..-0.800....-0.800..0.800..0.800 equil....0.34......0......0.800..0.800 ...
Sunday, October 30, 2011 at 9:10pm by DrBob222

Biochem
10ml of HCl acid titrate with 9.9ml of NaOH. What is the mass in grams of HCl?
Tuesday, August 3, 2010 at 5:04pm by Amrik

Chemistry
For a), calculate moles HCl (Moles = M x L) and see which is in excess. Since both HCl and NaOH are strong electrolytes, their molarity will be the H^+ (or OH^- if NaOH is in excess) and pH can be determined from that. For b), it is more complicated than that. Acetic acid and ...
Tuesday, August 11, 2009 at 7:28pm by DrBob222

College Chemistry
The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated ...
Tuesday, October 19, 2010 at 11:10pm by James

AP Chemistry
You have mols HCl = M x L = ? It will take the same number of mols to neutralize HCl since reaction ratio is 1 mol NaOH to 1 mol HCl.
Monday, March 3, 2014 at 4:34pm by DrBob222

Chemistry eq
mL HCl x M HCl = mL NaOH x M NaOH.
Wednesday, March 27, 2013 at 3:37pm by DrBob222

Chemistry - Acid Base Titration
When you complete a acid base titration of NaOH and HCl and how to you find the molarity/concentration of HCl. I used 9 mL of HCl with 50 mL of water. But when solving for concentration, do I use 9 mL or 59 mL (water + HCl)? Also, does the water in the HCl affect the outcome ...
Thursday, January 31, 2008 at 8:27pm by Steve

Chemistry
A). The pH of PURE water is 7.0. Distilled water CAN be less than 7.0 if it has absorbed some CO2 from the air. B) The 6.0 M HCl has been diluted 1 mL to 41 mL; therefore, molarity of HCl is 6.0 x (1/41) = ??. HCl is a strong electrolyte and ionizes 100%; therefore, the H^+ is...
Thursday, November 1, 2007 at 9:35pm by DrBob222

CHEMISTRY (WEBWORK)
What is the pH of the solution created by combining 1.20 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)? mL NaOH pH w/ HCl pH w/ HC2H3O2 1.20 ? ? Complete the table below: What are the pH values if you take into account ...
Monday, July 12, 2010 at 6:19pm by Anonymous

Chemisty (please read soon)
which will become a buffer in 1L of H2O? a) 0.3 mole KOH & 0.3 mole HBr b) 0.5 mole NH3 & 0.5 mole HCl c) 0.2 mole NaCl & 0.3 mole HCl d) 0.2 mole NaOH & 0.2 mole HBr e) 0.4 mole HC2H3O2 & 0.2 mole NaOH I think that the answer is e. Is that correct?
Sunday, April 29, 2012 at 11:03pm by Zac

Chem
NaOH + HCl ==> NaCl + H2O moles NaOH initially = in the problem. moles HCl initially = M x L = ?? Subtract the two (the smaller from the larger) and the difference is the amount of the larger one in excess. Then H^+ or OH^- = (moles larger/total L) = ?? Convert that answer ...
Sunday, November 28, 2010 at 9:00pm by DrBob222

ap chemistry
Since HCl and NaOH react in a 1:1 ratio, 0.200 L x 2.2 M NaOH = 0.440 mols will react with 0.200 x 3.9 = 1.17 mols HCl to form (ONLY) 0.44 mol NaCl. M = mols/L soln (careful--the solution volume will be 300 + 200 = 500 mL or 0.5L).
Tuesday, March 5, 2013 at 8:14pm by DrBob222

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