Search: what volume of 5M HNO3 is required to prepare 1.0L of 0.05M HNO3

Number of results: 25,283

johnson
Work these titration calculations: 1. A titration of 15.0 cm3 of household ammonia, NH3, required 38.57 cm3 of 0.78M HCl. Calculate the molarity of the ammonia. 2. What volume of 0.5M HNO3 is required to neutralize 25 cm3 of a 0.2M NaOH solution? 3. ...
Monday, June 18, 2012 at 8:13pm by Lemun

Chemistry
What volume of 0.5M HNO3 is required to neutralize 25 cm3 of a 0.2M NaOH solution? please show work and detail.
Thursday, January 15, 2009 at 12:50am by Paige

Science(Chemsitry)
HNO3 used as a reagent has specific gravity of 1.42g/ml and contains 70% by strength HNO3. Calculate a)Normality Of Acid b)Volume of acid that contains 63g pure acid c)Volume of water required to make 1N solution from 2ml conc.HNO3
Thursday, June 16, 2011 at 2:43am by Atul

Chemistry 2
HNO3 + KOH ==> KNO3 + H2O a)HNO3 is 100% ionized; therefore, pH = -log(H^+) = -log(HNO3) = ? b) mols HNO3 = M x L = ? mols KOH added = ? mols HNO3-mols KOH = mols HNO3 remaining. M HNO3 remaining = mols HNO3/total volume. Don't forget total volume will be amount ...
Tuesday, April 2, 2013 at 10:44pm by DrBob222

chemistry
What volume of 6.58 M HNO3 is required to prepare 671 mL of a 2.7 M HNO3 solution?
Thursday, September 13, 2012 at 4:56pm by cheri

chemistry
What will be the volume of 8.52 M HNO3 required to prepare 763 mL of a 1.5 M HNO3 solution?
Sunday, April 10, 2011 at 8:22pm by Anonymous

chemistry
A volume of 29.62 ± 0.05 mL of HNO3 solution was required for complete reaction with 0.8896 ± 0.0008 g of Na2CO3, (FM 105.988 ± 0.001). Find the molarity of the HNO3 and its absolute uncertainty. I have the molarity of HNO3 = 0.5667
Thursday, August 30, 2012 at 2:52pm by Amanda

Chemistry
A volume of 29.62 ± 0.05 mL of HNO3 solution was required for complete reaction with 0.8896 ± 0.0008 g of Na2CO3, (FM 105.988 ± 0.001). Find the molarity of the HNO3 and its absolute uncertainty. I have the molarity of HNO3 = 0.5667
Wednesday, August 29, 2012 at 10:39pm by Amanda

Chemistry
What volume of 5.26 M HNO3 is required to prepare 236 mL of a 1.4 M HNO3 solution? Answer in units of mL
Thursday, September 15, 2011 at 8:28pm by Anonymous

AP Chemistry
What volume of 3.16 M HNO3 is required to prepare 524 mL of a 0.2 M HNO3 solution? Answer in units of mL.
Wednesday, September 19, 2012 at 8:27pm by Matt

ap chemistry
What volume of 6.58 M HNO3 is required to prepare 671 mL of a 2.7 M HNO3 solution? Answer in units of mL
Thursday, September 13, 2012 at 5:03pm by cheri

AP Chemistry
What volume of 6.48 M HNO3 is required to prepare 301 mL of a 1.2 M HNO3 solution? Answer in units of mL.
Sunday, October 24, 2010 at 2:33pm by Anonymous

Chemistry II
What volume of .0500 M calcium hydroxide is required to neutralize 38.50 mL of .0400 M nitric acid? 1. Write the equation. 2. M HNO3 x L HNO3 = mols HNO3. 3. Use the equation to convert mols HNO3 to mols Ca(OH)2. 4. Now use M x L = mols to calculate volume (L) Ca(OH)2. I ...
Wednesday, April 25, 2007 at 6:23pm by Jayd

chemistry
An HNO3 solution has a pH of 3.04. What volume of 0.015 M LiOH will be required to titrate 89.0 mL of the HNO3 solution to reach the equivalence point?
Thursday, January 5, 2012 at 8:11pm by Anonymous

math,science,lab
HNO3+NaOH=NaNO3+H2O No. of moles of NaOH = 0.011*0.1 = 0.0011M Therefore no. of moles of HNO3 in 5ml. = 0.0011M Concentration of diluted HNO3 = 0.0011/0.005=0.22N Volume of 15.8N HNO3 required = x litre. 0.22N*1 litre+15.8x = 0.25(1+x) Solve for x to get x=3/1555 =0.00193 l. =...
Monday, August 23, 2010 at 6:21pm by MathMate

college chemistry
Suppose you have a 0.200 M solution of the nitrogen-containing weak base NX. Suppose you wish to titrate 25 mL of this 0.200 M NX solution with a 0.100 M solution of the strong acid HNO3. Given that the Kb value of NX is 6.50x10-5, complete each of the following: a) What ...
Wednesday, April 21, 2010 at 5:58pm by Aubree

chemistry
8.52M X V = 1.5M X 763mL (C1V1 = C2V2) i.e. Mass of HNO3 in Left = Mass of HNO3 in right V = (1.5M x 763mL)/ 8.52M = 134.3309mL Vol of water = 763 - 134.3309 = 628.6690mL i.e you add 134.3mL of 8.52M HNO3 to 628.7mL of water.
Sunday, April 10, 2011 at 8:22pm by Alien

CHEMISTRYY!
Determine if HNO3 can dissolve in the following metal: 1) Write a balanced chemical reaction showing how the 2.09g Cu dissolves in HNO3. I had put down: Cu(s) + 4HNO3(aq) ——> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) but it's wrong. 2) Determine the minimum volume ...
Sunday, March 31, 2013 at 12:47am by Lisa

Chemistry
What volume of 0.105 M HNO3, in milliliters, is required to react completely with 1.40 g of Ba(OH)2? 2 HNO3(aq) + Ba(OH)2(s) Ba(NO3)2(aq) + 2 H2O(l)
Thursday, September 23, 2010 at 8:12pm by Noelle

chemistry
Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3) is added to the acidified water. What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 1...
Tuesday, October 12, 2010 at 8:30pm by Anonymous

chemistry
A volume of 100mL of a 0.800 M HNO3 solution is titrated with 0.640 M KOH. Calculate the volume of KOH required to reach the equivalence point.
Monday, August 6, 2012 at 7:13pm by LL

Chemistry
moles first HNO3 = M x L = ?? moles second HNO3 = M x L = ?? molarity of final solution = total moles/total volume. Since HNO3 is a strong acid (100% ionized) the pH = -log(H^+) and (H^+) (HNO3)
Monday, April 5, 2010 at 3:00pm by DrBob222

chemistry
how preapare 30.0ml of 0.800m HNO3 FROM A STOCK SOLUTION OF 4.00M HNO3 WHAT VOLUME IN ML OF THE 4.OOM HNO3 SOLUTION WILL YOU NEED?
Sunday, April 10, 2011 at 8:22pm by Anonymous

Chemistry
There are a few ways to do these and you may well have a standard formula. However, you might like to try this approach for these problems. The 1.00 L of 0.18 M HNO3 contains 1.00 L x 0.18 mole L^-1 = 0.18 moles of HNO3. So we need 0.18 moles of HNO3 from the stock solution. ...
Wednesday, October 1, 2008 at 12:38am by Dr Russ

chemistry
What volume of .200M NaOH will be required to react completely with 32 mL of .15M HNO3
Tuesday, April 20, 2010 at 12:12am by joe

Chemistry
The easiest way to explain this (but perhaps the long way around) is to first convert to molarity for both HCl and HNO3. For HCl: 1.19 g/mL x 1000 mL x 0.38 x (1 mol/molar mass HCl) = mols HCl/L = M For HNO3: density g/mL x 1000 mL x 0.70 x (1 mol/molar mass HNO3) = moles HNO3...
Monday, May 21, 2012 at 8:44pm by DrBob222

chemistry
what volume (in ML) of a 0.150 M HNO3 solution is required to completely react wtih 35.7 mL of a 0.108 M Na2CO3 solution according to the following balanced chemical equation? Na2CO3(aq) + 2 HNO3(aq) --> 2NaNO3(aq) + H2O(l) then, in the reaction above, what mass (in ...
Monday, June 21, 2010 at 2:53pm by samantha

chemistry
what volume of 1.5M NaOH would be required to neutralize 0.65g of pure aspirin?
Tuesday, January 11, 2011 at 6:37pm by kelis

Chemistry
What volume of NaOH is required to neutralize 50mL of 0.5M phenol? So this is just a small calculation in a complex problem, and I would just like someone to check my work so I don't mess up the entire problem based on this calculation. So mol phenol= molarity x volume = (...
Friday, November 19, 2010 at 7:21pm by Jon

Chemistry
How many grams of CaCl2 would be required to produce a 3.5M(molar) solution with a volume of 2.0L?
Saturday, April 27, 2013 at 1:27pm by Sunny

chemistry
How many milliliters of 16.0 M HNO3 stock solution wouuld be required to prepare 100.0mL of 3.00 M HNO3? Use the formula M1V1=M2V2
Monday, January 23, 2012 at 7:56pm by missy

chemistry
what volume of water should be added to 300ml of HNO3 0.25M to obtain HNO3 0.2M?
Friday, September 7, 2012 at 10:44am by gaby

Chemistry
What is the minimum volume of 6.5M HCl required to completely dissolve 24.0g of magnesium metal?
Thursday, November 17, 2011 at 12:54pm by Lorena

physics
4.5/m^3 just is not volume. Assume it meant 4.5m3. Then energy= heatvalue*volume=39MJ/m^3*4.5m^3=you do it.
Thursday, July 22, 2010 at 1:43am by bobpursley

Chemistry
A 0.105-L sample of an unknown HNO3 solution required 36.9 mL of 0.200 M Ba(OH)2 for complete neutralization. What was the concentration of the HNO3 solution?
Sunday, October 14, 2012 at 10:45pm by Sarah

chemistry
A 0.115-L sample of an unknown HNO3 solution required 31.1 mL of 0.100 M Ba(OH)2 for complete neutralization. What was the concentration of the HNO3 solution?
Saturday, July 7, 2012 at 11:10am by Anonymous

chemistry
2HNO3 + Ca(OH)2 ==>Ca(NO3)2 + 2H2O Moles HNO3 initially = M x L Moles Ca(OH)2 required is 2 x moles HNO3 (because o the equation 1 mol Ca(OH)2 = 2 moles HNO3). Then moles Ca(OH)2 = L x M You know moles and M, calculate L, then multiply by 1000 to convert to mL.
Wednesday, September 30, 2009 at 1:40pm by DrBob222

chemistry
its actually the other way around, u need to figure out what volume u need of the .5M, e.g., if u want to make 500ml of it then u wud use c1vi=c2v2 so .5L X .5M = xL X 6M making xL subject of the formula u wud then have the volume of ^M NaOH u wud need to put in 500ml to get a...
Thursday, March 17, 2011 at 4:05pm by mai dee

Chemistry
How concentrated is the "concentrated" HNO3? If you are talking about commercial grade conc HNO3, it has a density of about 1.4 g/mL and it is about 68% by weight HNO3. You need to confirm these values from your text or notes and use those numbers instead of these ...
Thursday, September 6, 2012 at 9:18am by DrBob222

chemistry
To what volume should you dilute 48mL of a 13M stock HNO3 solution to obtain a 0.122 HNO3 solution?
Saturday, October 2, 2010 at 6:11pm by Anonymous

Chemistry 103
To what volume should you dilute 50ml of a 13M stock HNO3 solution to obtain a 0.131M HNO3 solution?
Sunday, October 7, 2012 at 3:42am by YeJi

chemistry
HNO3 + NaOH ==> NaNO3 + HOH You construct the table. mols NaOH = M x L = ?? The equation tells you it is 1 mol NaOH to 1 mol HNO3; therefore. mols NaOH = mols HNO3 Then M HNO3 = mols HNO3/L HNO3. Yo have mols and you have L. Calculate M HNO3.
Sunday, May 11, 2008 at 12:25pm by DrBob222

Chemistry
HNO3 is a strong acid; it ionizes 100%. moles HNO3 = grams/molar mass. M HNO3 = moles/L soln. pH = -log(HNO3).
Monday, January 24, 2011 at 8:15pm by DrBob222

chemistry
26.5 moles of a .2 M aqueous solution of NaOH is required to titrate 50 ml of an aqueous solution of HNO3, what is the concentration of HNO3. I don't want the answer, I want to know how to do it.
Monday, March 14, 2011 at 5:14pm by Daniel

chemistry
Calculate the volume of a 9.00 M HNO3 stock solution that must be used to prepare 450 mL 0f a 1.80 M HNO3 solution.
Wednesday, May 7, 2008 at 9:04pm by katie

chemistry
What volume of 16M HNO3 is required to dissolve 0.50g of Cu metal in the following reaction? Cu(s) + 4HNO3(aq) ---> Cu(NO3)2 + 2H2O + 2NO2
Thursday, February 3, 2011 at 8:41pm by Alex

chem
A 75.0 mL volume of 0.200 M NH3 (Kb=1.8x10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3.
Wednesday, April 20, 2011 at 1:23pm by Mike

chem
A 75.0 mL volume of 0.200 M NH3 (Kb=1.8x10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3.
Wednesday, April 20, 2011 at 1:11pm by Mike

calc 3
I'll do the volume. You should be able to get the others. If not, come back and we can help you get unstuck. v = lwh dv/dt = wh dl/dt + lh dw/dt + lw dh/dt plugging in the numbers, dv/dt = 5m*5m*(6m/s) + 7m*5m*(6m/s) + 7m*5m*(-4m/s) = 150+210-140=220 m^3/s
Friday, September 21, 2012 at 4:34pm by Steve

chemistry
Determine the minimum volume of 6.40M HNO3 required to dissolve a 2.40g sample of Cu. 2NO3-(aq)+8H+(aq)+3Cu(s)-->2NO(g)+4H2)(l)+3Cu2+(aq)
Wednesday, April 28, 2010 at 12:35pm by Catalina

Chemistry
Write the equation and balance it. HNO3 + NaOH ==> NaNO3 + H2O moles NaOH = M x L = ?? Using the coefficients in the balanced equation, convert moles NaOH to moles HNO3. Since the ratio is 1:1, that means moles NaOH = moles HNO3. M HNO3 = moles HNO3/L HNO3.
Tuesday, June 7, 2011 at 7:03pm by DrBob222

Chemistry
HNO3 + NaOH ==> NaNO3 + H2O mols NaOH = M x L = ? Look at the equation. It is 1:1 for base/acid so mols HNO3 = mols NaOH The M HNO3 = moles HNO3/L HNO3.
Sunday, March 25, 2012 at 9:34pm by DrBob222

Chemistry
.5g Cu is .000787 moles Cu 16M HNO3 is 16 moles/L You need 2 moles of HNO3 for each mole of Cu, so that's .00157 moles HNO3 .00157 mole / 16mole/L = .0000981 L = .0981mL Seems like an awfully small volume. Better check my math.
Monday, February 25, 2013 at 5:18pm by Steve

Chem 1
Calculate the molarity of the stock solution. 1.4 g/mL x 1000 mL x 0.63 x (1/molar mass HNO3) = ? M HNO3. Then use the dilution formula of c1v1 = c2v2 c = concn v = volume
Wednesday, December 5, 2012 at 4:03pm by DrBob222

Chemistry
Given the following chemical equation: 3 Cu + 8 HNO3 = 3 Cu(NO3)2 + NO + 4 H2O. How many moles of HNO3 are required to react with 6 moles of Cu?
Monday, July 14, 2008 at 2:01pm by Persia

Chemistry
3HNO3 + Al(OH)3 ==> Al(NO3)3 + 3H2O How many mols Al(OH)3 do you have? That is M x L = ? So how many mols HNO3 are needed to neutralize it. The equations tells you moles HNO3 = 3* moles Al(OH)3. Then M HNO3 = moles HNO3/L HNO3. You have M and moles solve for L HNO3 an ...
Friday, February 17, 2012 at 4:16pm by DrBob222

Chemistry
If 0.630 grams of HNO3 (molecular weight 63.0) are placed in 1 liter of distilled water at 25 degrees C, what will be the pH of the solution? (Assume that the volume of the solution is unchanged by the addition of the HNO3.) A. 0.01 B. 0.1 C. 1 D. 2 E. 3
Monday, January 24, 2011 at 8:15pm by Sharon

chemistry
What volume of .101 M HNO3 is required to neutralize each of the following solutions? there are four and i got them all right but this one... 51.1 mL of .127 M NH3 i got 193 mL can someone please help???
Tuesday, March 10, 2009 at 4:26pm by lyne

Titration/Acid-base chem
a .4000 M solution of nitric acid is used to titrate 50.00 mL of .237 M barium hydroxide (Assume that volumes are additive). a) Write a balanced net ionic equation for the reaction that takes place during titration. b) what are the species present at the equivalence point? c) ...
Sunday, May 6, 2007 at 5:16pm by Keith

math 12
the height of a ball is modelled by the equation h(t)= 4sin (8 pie t)+ 6.5 where h(t) is in metres and t is in seconds. what are the highest and lowest points the ball reaches? a) 10.5 m and 6.5m b) 10.5m and 2.5m c) 6.5m and 2.5m d) 14.5m and 6.5 m
Wednesday, May 8, 2013 at 9:31pm by i hate math part 2

Chemistry
2.5 l of 0.1M solution contains 0.25 moles. Volume of 5.5M stock solution required = 0.25/5.5 * 1000 ml
Sunday, December 5, 2010 at 12:55am by MathMate

Chemistry
1 mol of HNO3 will neutralise 1 mol of NaOH since concentration of HNO3 is half that of NaOH, volume will have to double. So 600ml
Saturday, October 9, 2010 at 11:39am by Anonymous

chemistry
what volume of a 2.5m stock soltio of acetic acid (HC2H3O2) is required to prepare 100.0 mililiters of a 0.50m acetic acid solution?
Wednesday, January 23, 2013 at 10:07am by Anonymous

chemistry
NO2 is not the anhydrous form of HNO3. N2O5 is. When NO2 is dissolved in water a mixture of HNO2 and HNO3 is produced. Commercially, O2 is added to oxidize the HNO2 to HNO3. Since the HNO3 produced is an aqueous solution, I don't understand calculating mols of a gas. ...
Wednesday, April 16, 2008 at 12:01pm by DrBob222

Food Analysis
1.If 0.5l of 5M solution of CU(NO3) is diluted to a volume of 0.80l by adding water, what is the molarity of the resulting diluted solution? 2.How many ml of water will be required to dilute 11ml of 0.45Macid solution to a molarity of 0.1M? 3.Calculate the weight CuSO4.5H2O ...
Tuesday, March 8, 2011 at 9:07am by Sarah

AP Chem
3 NO2(g) + H2O(g) 2 HNO3(g) + NO(g) At constant temperature and pressure, what is the maximum volume, in liters, of HNO3(g) that can be made from 10.39 L of NO2(g) and 15.53 L of H2O(g)?
Monday, June 18, 2012 at 9:05pm by Nihar

chemistry
The sample has a mass of 116.9g. If it is 70% HNO3 (by mass but the post doesn't say that), then the mass of HNO3 is that 116.9 g is 116.9*0.70 = ? grams HNO3. Then moles HNO3 = grams HNO3/molar mass HNO3.
Monday, December 5, 2011 at 3:02pm by DrBob222

Chemistry
How many mL of 3.00M HNO3 would you need to make exactly 100mL of 0.83 HNO3 by dilution with water? (The FM of HNO3 = 63.0.)
Wednesday, March 14, 2012 at 10:25pm by Lauren

Chemistry
Which of the following will buffer near pH=9? a. 0.5M sodiumacetate/0.5M acetic acid b. 0.5M ammonium chloride/0.5M ammonia c. 0.5M sodium dihydrogen phosphate/0.5M hydrogen phosphate i think a) 0.5M sodiumacetate/0.5M acetic acid will buffer near pH=9
Wednesday, October 17, 2012 at 8:59pm by Cristian

chemistry
A 1.00 L volume of 0.609 M HNO3 is condensed to a volume of 0.750 L, calculate the molarity (M) of H+ in the new solution
Sunday, March 28, 2010 at 3:17am by eng

chemistry
Which 2.5. There are two 2.5. One is 2.5M and one is 2.5L. The 2.5M comes from the 6L of 2.5M solution that you are preparing. The 2.5L is the volume of the 2M solution and the 4M solution that you are to mix together to obtain the 6L of 2.5M solution. HOWEVER, this is not the...
Wednesday, May 11, 2011 at 6:13pm by DrBob222

Chemistry Help Please
i do not understand how to solve this problem, please help 10.0mL 0.5M sulfuric acid can neutralize what volume of 0.5M ammonium hydroxide?
Saturday, March 31, 2012 at 7:08pm by Robert

chemistry
2HNO3 + Ba(OH)2 ==> Ba(NO3)2 + 2H2O mols Ba(OH)2 = M x L = ? convert mols Ba(OH)2 to mols HNO3 using the coefficients in the balanced equation. That is mols HNO3 = 2*mols Ba(OH)2 Then M HNO3 = mols HNO3/L HNO3.
Saturday, July 7, 2012 at 11:10am by DrBob222

chemistry
First calculate the percent HNO3 in conc HNO3. Do you have the percent? Most concn HNO3 is 68% by weight HNO3. Then 500 mL x 0.20 = ?mL x 0.68.
Thursday, August 30, 2012 at 3:25pm by DrBob222

Chemistry
Convert pH to (H^+) by pH = -log(H^+) Since there is 1 mol H^+ in 1 mol HNO3, then that is the concn of HNO3 in moles/L. mols in 248.6 mL = M HNO3 x L HNO3 and g = mols x molar mass.
Tuesday, February 28, 2012 at 7:26pm by DrBob222

Chemistry
Ca(OH)2 + 2HNO3 ==> 2H2O + Ca(NO3)2 mols Ca(OH)2 = grams/molar mass moles HNO3 = twice that (from the balanced equation). M HNO3 = mols HNO3/L HNO3. You know M and mols, solve for L and convert to mL.
Wednesday, February 29, 2012 at 2:27pm by DrBob222

Chemistry
How many mols KOH do you have? That's mols KOH = M x L = ? How many mols HNO3 will that neutralize. The same number since the equation is 1 mol HNO3 to 1 mol KOH. M HNO3 = mols HNO3/L HNO3.
Tuesday, October 23, 2012 at 6:37pm by DrBob222How

Chemistry
How many moles of HNO3 are required to make 250mL of a 2.4M solution? How many grams of KOH are required to make 125mL of a .50M solution?
Wednesday, March 4, 2009 at 8:43pm by Ali

Chem
2HNO3 + Ca(OH)2 ==> Ca(NO3)2 + 2H2O mols Ca(OH)2 = M x L = ? mols HNO3 = twice that (look at the coefficients). M HNO3 = mols HNO3/L HNO3.
Wednesday, June 13, 2012 at 11:29pm by DrBob222

Chemistry
10% v/v is 10 mL/100 mL soln but I think 10% HNO3 means 10g HNO3/100 mL solution unless you want 10% HNO3 mass percent which is 10 g HNO3/100 g solution. To any of these, however, you must know the concn of the HNO3 you're starting with.
Sunday, February 3, 2013 at 6:17am by DrBob222

chemistry
One liter of approximetely 0.25N HNO3 has been prepared. Upon titration it was found that 5.0 ml of the acid required 11.0 ml of 0.10N NaOH for neutrality. How much concetrated HNO3 at 15.8N must be added to one liter to make it exactly 0.25N?
Wednesday, September 8, 2010 at 8:52pm by sp

chemistry
5M*volume*molmassNaOH=50 solve for volume
Wednesday, March 30, 2011 at 8:21pm by bobpursley

Chemistry
You must mean HNO3 since there is no such thing as hno3. When adding AgNO3 to a solution to test for Cl^-, you acidify with HNO3 to make sure the soln is acid enough that AgOH does not ppt.
Wednesday, May 25, 2011 at 5:58pm by DrBob222

chemistry
dry gaseous hcl contained in volume of 1L at STP is dissolved in 200ml of 0.5M barium hydroxide soltion. How many mol of 0.5M hcl would be needed to neutralise the resulting solution?
Monday, April 2, 2012 at 9:56pm by mob

chemistry,math
One liter of approximetely 0.25N HNO3 has been prepared. Upon titration it was found that 5.0 ml of the acid required 11.0 ml of 0.10N NaOH for neutrality. How much concetrated HNO3 at 15.8N must be added to one liter to make it exactly 0.25N?
Monday, August 23, 2010 at 6:56pm by jc

Chemistry
How many mL of concentrated HNO3 (conc. HNO3 is 16 Molar)will be needed to make 1.25 Liters of 9 Molar HNO3?
Wednesday, December 5, 2012 at 10:28pm by Anonymous

chemistry
Copper reacts with nitric acid according to the following reaction: 3 Cu (s) + 8 HNO3 (aq) --> 3 Cu(NO3)2 (aq) + 2 NO (g) + 4 H2O (l) If an pre 1982 copper penny contains 3.10 grams of copper, what volume of 8.00 M nitric acid is required to exactly consume it? What ...
Sunday, November 7, 2010 at 7:16pm by Christy

PHYSICS - PLEASE HELP
KE = 0.5m*V^2. KE2/KE! = 0.5m(20)^2/0.5m*(10)^2 = 4. Note: 0.5m cancels
Wednesday, November 28, 2012 at 7:45am by Henry

calc/physics
A force of 250 N is required to stretch a spring 5m from rest. Using Hooke's law, F=kx, how much work, in joules, is required to stretch the spring 7m from rest? The energy required scales with x^2. Multiply 250 J by (7/5)^2.
Monday, April 23, 2007 at 3:46pm by Mischa

math,science,lab
One liter of approximetely 0.25N HNO3 has been prepared. Upon titration it was found that 5.0 ml of the acid required 11.0 ml of 0.10N NaOH for neutrality. How much concetrated HNO3 at 15.8N must be added to one liter to make it exactly 0.25N?
Monday, August 23, 2010 at 6:21pm by jc

Chemistry
g HNO3 = mols x molar mass = ? That is ?g HNO3/150 mL so ?g x (1000/150) = xg HNO3/L.
Wednesday, June 13, 2012 at 9:30pm by DrBob222

chemistry
Frankly, I don't think the problem is worded very well. This is an example of a problem in which the unknown amount of Mg(OH)2 is treated with a known amount of HNO3, which happens to be an excess. Then we determine the excess, subtract from the initial amount HNO3 there, ...
Wednesday, November 17, 2010 at 4:06pm by DrBob222

Chemistry
3 NO2(g) + H2O(g) 2 HNO3(g) + NO(g) At constant temperature and pressure, what is the maximum volume, in liters, of HNO3(g) that can be made from 10.39 L of NO2(g) and 15.53 L of H2O(g)? That is the entire question and this is AP Chem but gas stoichiomatry from regular chem. I...
Monday, June 18, 2012 at 8:55pm by Nihar

chemistry
mols HNO3 = grams HNO3/molar mass HNO3 Solve for mols HNO3. Then mols = M x L. You know M and mols, solve for L and convert to mL.
Sunday, October 28, 2012 at 10:10am by DrBob222

AP Chemistry
How many moles do you want? That's M x L = ? Then M HNO3 = mols HNO3/L HNO3. You know M and mols. Solve for L and convert to mL.
Wednesday, September 19, 2012 at 8:27pm by DrBob222

chemistry help
Nitric acid,HNO3, is available ata a concentration of 16 M. how much would react with 5.58 g of KOH acording to the following equation? HNO3+KOH-H2O+KNO3 dont understand? does not give me a volume amount to work with and I really dont understand how to solve it
Sunday, November 21, 2010 at 6:17pm by nicole

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