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April 20, 2014

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

Number of results: 20,401

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 HNO3 you ...
Tuesday, April 2, 2013 at 10:44pm by DrBob222

johnson
Work these titration calculations: 1. A titration of 15.0 cm3of household ammonia, NH3, required 38.57 cm3of 0.78M HCl. Calculate the molarity of the ammonia. 2. What volume of 0.5M HNO3is required to neutralize 25 cm3of a 0.2M NaOH solution? 3. Calculate the volume of 0....
Monday, June 18, 2012 at 8:13pm by Lemun

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

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

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
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
For both nitric acid and sodium hydroxide, the acid hydrogen equivalence factor is 1. That is: 1N=1M. Given: 22mL HNO3 neutralises 20mL, 0.5N NaOH, via the stoichiometry: HNO3 + NaOH = NaNO3 + H2O Molar Mass of HNO3 is 63.012960.00004 g/mol. Let: c be the concentration of ...
Sunday, September 8, 2013 at 3:08am by Graham

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
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 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
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
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
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
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 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

AP Chemistry- Acids
pH = -log(HNO3) -1.39 = log(HNO3) I found HNO3 approximately 0.05 but you need to do it more accurately. Then mol HNO3 = M x L = ? mols HCl = M x L total mols H^+ = mols HCl + mols HNO3. volume = 145 mL + 493 mL = ? M new solution = total mols/total liters. Then pH = -log(H^+)
Wednesday, February 12, 2014 at 6:27pm by DrBob222

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

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
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
The density of 19.0% by mass of nitric acid, HNO3 is 1.11 g cm-3. Calculate the volume (dm3) of acid needed to prepare 2.00 dm3 of 3.00 mol dm-3 HNO3 solution. (FW HNO3 = 63 g/mol)
Friday, March 28, 2014 at 3:56am by h

Chemistry
find the mole for HNO3 using n = MV where M is the molarity and V is the volume in Liters. then use the balance equation; KOH + HNO3 --> KNO3 + H2O the reaction is 1:1 so the mole you calculated for HNO3 is also the mole for KOH. i.e. mole KOH = mole HNO3. then convert the ...
Monday, June 10, 2013 at 1:29pm by bonjo

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 estimates. ...
Thursday, September 6, 2012 at 9:18am by DrBob222

Chemistry
A and B are ok. I think C is incorrect. If the soln is 71.5%, then you are right that 1.13 mol HNO3. 100 g soln = 71.5g HNO3 = 2.85g H2O (I think you converted to volume). Then XHNO3 = 1.13 mols HNO3/(1.13+2.85) = about 0.4 or so.
Sunday, May 26, 2013 at 10:30pm 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
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 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

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 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

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
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
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
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

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

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

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 2, 2014 at 12:43am by Billy Bob Reynolds

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

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
1. calculate the volume of concentrated HNO3 (68%)that is needed to prepare stock solution 0.25M in 1000mL volumetric flask. (density HNO3 = 1.513 g/cm^3) 2. from above stock solution, determine volume needed to dilute to 500mL volumetric flask that contained 10 times dilution.
Wednesday, July 10, 2013 at 12:25pm by Susan

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
.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

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

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 of 6.3M HNO3 ...
Sunday, March 31, 2013 at 12:47am by Lisa

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
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
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
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

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

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
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
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
1. What molarity is needed so that 5mL diluted to 475 mL will yield 0.1M? For this one I used M1V1=M2V2 and got 9.5M just checking to see if I did that right. 2. How much 2.5 HNO3 can be made from 7.0mL of a 16.0M HNO3 soltuion? I tried using M1V1=M2V2 for this one too but ...
Sunday, June 2, 2013 at 1:47pm by helppp please

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
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
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
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 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
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
Dr. Bob222 gave you the setup to calculate the grams of CaCl2. But I will go into a little bit more detail and maybe this will help: Molarity=Moles/Volume (L) The question tells you that you need need a total of 2L, but you don't know how many moles are in a 3.5M solution with...
Saturday, August 17, 2013 at 5:03pm by Devron

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
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
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
2HNO3 + Ba(OH)2 ==> 2H2O + Ba(NO3)2 mols Ba(OH)2 = M x L = ? Use the equation coefficients to convert mols Ba(OH)2 to mols HNO3. Note: that's mols HNO3 = 2*mols Ba(OH)2. Then M HNO3 = mols HNO3/L HNO3. You know L and mols, solve for M.
Saturday, November 9, 2013 at 3:03pm by DrBob222

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
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

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
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
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
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
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
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

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

chemisty
How many mL of a 0.5M Ca(OH)2 solution are needed to neutralize 38mL of a 2M HNO3 solution?
Saturday, November 24, 2012 at 6:48pm by Boo Boo

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

Science
The reaction is 3 Cu + 8 HNO3 3 Cu2+ + 2 NO + 4 H2O + 6 NO3- First you need to determine the limiting reactant, Cu or HNO3. It looks like it is HNO3. There is only 0.06 moles of it.
Monday, November 7, 2011 at 6:02am by drwls

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
How many milliliters of a .5M HNO3 (aq) is needed to completely neutralize 100mL of a 0.10M KOH (aq)?
Wednesday, May 30, 2012 at 3:22pm by Kc

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

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
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
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

Physics URGENT HELP
I think I know what you were looking for. Starting off where Damon left off, Max acceleration occurs when the velocity=acceleration. Vi=0m/s^2 Vf=5m/s and a=5m/s^2 d=? Solve for d. Vf^2=Vi^2+2ad (5m/s)^2=0+2(5m/s^2)d 25=10d 25/10=d d=2.5m The runner establishes max ...
Thursday, August 29, 2013 at 6:12pm by Devron

Physics URGENT HELP
I think I know what you were looking for. Starting off where Damon left off, Max acceleration occurs when the velocity=acceleration. Vi=0m/s^2 Vf=5m/s and a=5m/s^2 d=? Solve for d. Vf^2=Vi^2+2ad (5m/s)^2=0+2(5m/s^2)d 25=10d 25/10=d d=2.5m The runner establishes max ...
Thursday, August 29, 2013 at 6:12pm by Devron

Chemistry, #4
Calculate the concentration of an aqueous HNO3 solution that has a pH=5.08. pH = 5.08. Convert that to (H^+). Since HNO3 is a strong acid and it is 100% ionized, (H^+) = (HNO3).
Friday, August 3, 2007 at 4:34pm by Taasha

Chemistry
USUALLY it is done this way but you need more info than 2mL conc HNO3. mass HNO3 = density in g/mL x mL x (%HNO3/100) = ?g Then mols = grams/molar mass.
Thursday, August 30, 2012 at 4:46pm by DrBob222

Chemistry
I assume the 0.0021 is M. mols KOH = M x L = ? mols HNO3 = mols KOH (from the coefficients in the equation.) M HNO3 = mols HNO3/L HNO3. You know mols and L, solve for M.
Thursday, March 21, 2013 at 1:26am by DrBob222

CHEMISTRYY!
If you posted the problem as written then it is not written very well. Your equation looks ok to me for concentrated HNO3. For dilute HNO3 it is 3Cu + 8HNO3==> NO etc. Perhaps the prof want dilute HNO3 used. For #2. mols Cu = grams/molsr mass Convert mols Cu to mols HNO3 ...
Sunday, March 31, 2013 at 12:47am by DrBob222

chemistry
How would you make up 255 mL of 0.150 M HNO3 from nitric acid that is 68.0% HNO3? The density of 68.0% HNO3 is 1.41 g/mL.
Saturday, July 30, 2011 at 12:31am by Henry

6th math
change the width to meters, 6.5m P=2l + 2w = 2*5m + 2*6.5m = 10m + you finish it.
Sunday, January 18, 2009 at 8:48pm by bobpursley

Chemistry -pls help urgent
I would start the HNO3 by determining the molarity of the HNO3. density = 1.42 g/mL x 1000 mL = 1420 grams. It is 69% by mass; therefore, the amount of HNO3 in that 1420 g is 1420 x 0.69 = 979.8 grams. How many moles is that? 979.8/molar mass = about 15.5 M Then mL x M = mL x ...
Tuesday, October 12, 2010 at 5:04pm by DrBob222

Science
You have a stock solution of 3.5M glucose. You need a working solution of 0.5M glucose in a volume of 400ml. Explain how you make the solution. Also what is the concentration of the dilution solution?
Monday, October 15, 2012 at 10:10am by Helper

chem
How much does a liter of solution weigh? It has a mass of 1.084 g/mL x 1000 mL = 1084 grams. There are 2.580 moles HNO3 in the 1084 g of solution; therefore, 2.580 x molar mass HNO3 = about 162 g HNO3. (You need to do it exactly). % HNO3 = (g HNO3/mass solution)*100 = about (...
Thursday, February 12, 2009 at 11:58pm 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 grams) ...
Monday, June 21, 2010 at 2:53pm by samantha

math
5m+6=-4 5m = -4 - 6 5m = -10 m = ? If you post your answer, we'll be glad to check it.
Monday, December 17, 2007 at 8:14pm by Ms. Sue

Chemistry
a). First, you omitted what you want t calculate!!! .......CH3NH2 + HNO3 ==> CH3NH3^+ + NO3^- mmoles CH3NH2 = 119.2 mL x 0.105 = ?? mmoles HNO3 = 49.1 x 0.255 = ?? Take a look at the numbers; I think the rounded numbers (to 3 s.f.) are equal and the pH (H^+) at the ...
Sunday, February 6, 2011 at 7:23pm by DrBob222

chem
For the reaction 3NO2 + H2O  2HNO3 + NO, how many grams of HNO3 can form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react? This is a limiting reagent problem. 1. Write the equation. You have done that and it is balanced. 2. Convert 1.00 g NO2 and 2.25 g H2O to mols. ...
Wednesday, February 28, 2007 at 4:31pm by meghan

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