Monday
April 21, 2014

Search: HNO3

Number of results: 1,075

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

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
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
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
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
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
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 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
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
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
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
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
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
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

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

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
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- 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

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

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
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

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

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

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

chemistry
Is that 15% w/w or w/v? If w/w, then 15% means 15 g HNO3 in 100 g solution or 15 g HNO3 in (15 g HNO3 + 85 g H2O). Convert 15g HNO3 to moles. moles = grams/molar mass. Convert 85 g H2O to moles. Then XHNO3 = moles HNO3/total moles. XH2O = moles H2O/total moles. Post your work ...
Tuesday, December 13, 2011 at 10:33pm by DrBob222

Chemistry
moles = grams/molar mass. Calculate moles HNO3. M = moles/L Calculate M Since HNO3 is a strong acid, the H3O^+ will be the same as the HNO3.
Monday, June 7, 2010 at 7:50pm by DrBob222

Chemistry
mols KOH = M x L = ? Look at the equation; it is 1:1, therefore, mols HNO3 = mols KOH. M HNO3 = mols HNO3/L HNO3.
Friday, October 19, 2012 at 1:06pm by DrBob222

CHEMISTRY
HOW YOU PREPARE 30.0ML OF 0.800M HNO3 FROM A STOCK SOLUTION OF 4.OOM HNO3? WHAT SOLUTION IN ML OF THE 4.OOM HNO3 SOLUTION WILL YOU NEED?
Sunday, April 10, 2011 at 9:00pm by SARAH

College Chemistry
Writ the equations and balance them. HNO3 + KOH ==> KNO3 + H2O 3HNO3 + Al(OH)3 ==> 3H2O + Al(NO3)3 millimoles KOH = mL x M = 45.0*0.667 = 30.015 Convert mmoles KOH to mmoles HNO3 using the coefficients in the balanced equation. That is done as mmoles HNO3 = mmoles KOH x...
Thursday, October 6, 2011 at 6:27pm by DrBob222

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
HNO3 + KOH ==> KNO3 + H2O How many moles do you have? That's M x L HNO3. Look at the coefficients in the balanced equation. 1 mol HNO3 = 1 mol KOH; therefore, mols HNO3 = moles KOH. M KOH = moles KOH/L KOH. You know M KOH and mols KOH; solve for L KOH.
Monday, August 6, 2012 at 7:13pm by DrBob222

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
It means you have 16 mol HNO3/L solution. The molar mass of HNO3 is abouat 63 so you have 16 x 63 grams HNO3/L.
Sunday, March 24, 2013 at 7:15pm 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
NaOH + HNO3 ==> NaNO3 + H2O mols HNO3 = M x L = ? mols NaOH = mols HNO3 (look at the coefficients in the balanced equation.) mols NaOH = grams/molar mass
Saturday, December 8, 2012 at 2:14am by DrBob222

chemistry
A commercial sample of concentrated aqueous nitric acid (HNO3) is 18.2% nitric acid base mass and has a density of 1.12 g/mL. (a) What is the molarity (M) of the HNO3 solution? (b) What is the molality (m) of the HNO3 solution? -------- I know that.... (a) molarity = moles of ...
Wednesday, January 21, 2009 at 7:54pm by Sarah

chemistry
I agree with your answer to (a) of 10.74. I agree with b and c. For D, H2NNH2 + HNO3 ==> H2NNH3+^ + NO3^- You had 0.1 L x 0.1 M = 0.01 moles H2NNH2. You added 0.06 L x 0.2 M = 0.012 moles HNO3. You had an excess of 0.002 mols HNO3 (just has you have it). So there is an ...
Sunday, July 26, 2009 at 2:14am by DrBob222

chemistry
density 1.42 g/mL. Then 1000 mL has a mass of 1.42 g/mL x 1000 = 1420 grams That is 70% HNO3 so g HNO3 is 1420 x 0.70 = about 994 g. The rest of it is water. g H2O = 1420-994 = about 426 g = 0.426 kg. mol HNO3 = 994/molar mass HNO3. m = mols HNO3/kg solvent.
Wednesday, October 16, 2013 at 11:24pm by DrBob222

chemistry
thanks for all this help! so for this one, 1 - it would be 0.108 x 35.7 = 3.86 moles of Na2CO3 2 - 2.86 moles Na2CO3 / 2 Moles HNO3 = 1.93 Moles HNO3. 3 - 1.93 Moles HNO3 x 0.150 M HNO3 = 0.290 L which would equal 290 mL. Is this the final solution? 4 - I need help with this ...
Monday, June 21, 2010 at 2:53pm by samantha

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
HNO3. H = +1. O = 3*-2=-6 N must be +5 for HNO3 to be zero. See the other post for NO2 of +4 for N.
Friday, November 18, 2011 at 10:12am by DrBob222

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

Chem 106
Calculate the grams of HNO3 in 35.0 ml of a 6.00 M HNO3 solution
Thursday, April 8, 2010 at 11:42pm by jessica

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
20% of HNO3 reacts with 10g of Caco3 by weight then find the quantity of HNO3?
Sunday, February 10, 2013 at 7:59am by Anand mishra

Chemistry
HNO3 + NaOH ==> NaNO3 + H2O moles HNO3 = M x L = 0.0136 moles NaOH = g/molar mass = 16/40 = 0.4 So all of the HNO3 will be used up and NaOH remaining will be 0.400 - 0.0136 = ?? and molarity = moles/L = ??
Monday, October 25, 2010 at 6:58pm by DrBob222

Chemistry
What is the percent N in HNO3? That's (14/63)*100 = about 22% or so. mols HNO3 = M x L = 5.0*0.500L = 2.5 mols. grams HNO3 = 2.5 mols x molar mass = about 160g. Then about 160 x 0.22 = ?. Don't forget I estimated these numbers.
Saturday, April 13, 2013 at 7:49pm by DrBob222

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
HNO3 is a strong acid; it is ionized 100%. Therefore, (HNO3) = (H^+) = 0.28 M. Convert to pH.
Sunday, March 14, 2010 at 5:52pm by DrBob222

chemistry
how would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3?
Wednesday, September 29, 2010 at 2:09am by Michael

chemistry
How many milliliter of conc. HNO3 would be necessary to prepare 500ml of 20% of HNO3 solution?
Thursday, August 30, 2012 at 3:25pm by Jake

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 help asap
how would you prepare 60.0 ml of 0.2 M HNO3 from a stock solution of 4.00 M HNO3?
Monday, February 6, 2012 at 8:20pm by Abdul

Chemistry
HNO3 is a strong acid meaning that it is 100% ionized. Therefore, pH = -log(HNO3)
Wednesday, June 5, 2013 at 10:57am by DrBob222

chemistry
How many milliliters of 0.524 M HNO3 contain 3.13 g HNO3?
Sunday, October 28, 2012 at 10:10am by bebo

Chemistry-gases
I would calculate mols HNO3 produced by 532 g NO2 and substitute into PV = nRT and solve for L HNO3 at the temperature and pressure. Then ppm = L HNO3/1,000,000 L air at 20C. 0.08E-6 = LHNO3 produced/x Solve for x = L air Check my thinking.
Thursday, March 1, 2012 at 7:26pm by DrBob222

Chemistry
mols KOH = M x L = ? mols HNO3 = mols KOH (look at the coefficients.) M HNO3 = mols HNO3/L HNO3.
Wednesday, January 23, 2013 at 7:45pm by DrBob222

Chemistry
Write and balance the equation. LiOH + HNO3 ==> LiNO3 + H2O How many moles HNO3 do you have? That's M x L = ? How many mols LiOH is that? Since 1 mol LiOH = 1 mol HNO3, mols LiOH = mols HNO3 (from the equation). mass LiOH = mols LiOH x molar mass LiOH.
Tuesday, June 5, 2012 at 3:23am by DrBob222

chemistry
A 116.9 g sample of nitric acid solution that is 70.0% HNO3 contains how many moles of HNO3? how did you get the answer
Monday, December 5, 2011 at 3:02pm by diana

CHEMISTRY
A 116.9 g sample of nitric acid solution that is 70.0% HNO3 contains how many moles of HNO3? how did you get the answer
Monday, December 5, 2011 at 4:39pm by diana

chemistry
A 116.9 g sample of nitric acid solution that is 70.0% HNO3 (by mass) contains how many moles of HNO3? how did you get the answer
Monday, December 5, 2011 at 5:03pm by DIANA

science
A solution of HNO3 has a pH of 4.5, What is the molarity of HNo3?
Tuesday, April 26, 2011 at 11:37am by Ray

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

organic chemistry
This is hardly organic chemistry. (HNO3) = 1.25E-3M. Since HNO3 is a strong acid (100% ionized), that means (HNO3) = (H^+); therefore, (H^+) = 1.25E-3 and pH = -log(H^+) = -log(1.25E-3) = ?? The answer is approximately 3
Monday, May 2, 2011 at 2:07pm by DrBob222

Chemistry
Convert 1.4 g Ba(OH)2 to moles. moles = grams/molar mass Using the coefficients in the balanced equation, convert moles Ba(OH)2 to moles HNO3. Finally, M = moles/L soln. You have M HNO3 and moles HNO3, solve for L.
Thursday, September 23, 2010 at 8:12pm by DrBob222

chemistry
How many milliliters of a stock solution of 12.0M HNO3 would you have to use to prepare 0.400M of 0.390 HNO3 ?
Saturday, September 25, 2010 at 4:01pm by riah

chemistry
Convert pH of 2.10 to (H^+) which is the same as (HNO3) since HNO3 is 100% ionized. Then the dilution formula is c1v1 = c2v2
Sunday, June 12, 2011 at 12:31am by DrBob222

Chemistry
In a 1.0x10^-6 M soltution of HNO3(aq), identify the relative molar amounts of these species. H2O , HNO3, H3O+,NO3-, OH-
Monday, October 17, 2011 at 10:34pm by Alexis Moran

CHEMISTRY
In a 1.0x10^-6 M soltution of HNO3(aq), identify the relative molar amounts of these species. H2O , HNO3, H3O+,NO3-, OH-
Monday, October 17, 2011 at 11:04pm by Alexis Moran

Chemistry
HNO3 is a strong acid. HCOOH is a weak acid. Therefore, the final H^+ concn will be that of HNO3 + that from HCOOH. You know the H^+ from HNO3 since that is a strong acid. That H^+ will act as a common ion to HCOOH. HCOOH ==> H^+ + HCOO^- Ka = (H^+)(HCOO^-)/(HCOOH) Set up ...
Thursday, October 7, 2010 at 6:28pm by DrBob222

chemistry
Convert 2.40 g Cu to moles. moles = grams/molar mass Using the coefficients in the balanced equation, convert moles Cu to moles HNO3. Molarity = moles/L. YOu know moles HNO3 and M HNO3, calculate L.
Wednesday, April 28, 2010 at 12:35pm by DrBob222

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

chem
NH3 + HNO3 ==> NH4NO3 Set up an ICE chart, determine which reagent is in excess after the addition of the HNO3, the pH from that.
Wednesday, April 20, 2011 at 1:23pm by DrBob222

Chemistry
First thing calculate the molarity of HCl and HNO3. HCl: 1.19 g/mL x 1000 mL x 0.38/molar mass HCl = approx 12M but you need to do it more accurately. HNO3: 1.42 g/mL x 1000 mL x 0.70/molar mass HNO3 = approximately 16M. mol H^+ from HCl = 50.3 x 12M = ? mol H^+ from HNO3 = 16...
Tuesday, February 28, 2012 at 7:25pm by DrBob222

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
If a sample of HNO3 is found to contain 8.44 10-2 mol of N atoms how many moles of HNO3 molecules are present? Express your answer in scientific notation.
Wednesday, April 3, 2013 at 9:51pm by Katie

Chemistry
In a 1.0 x10-6 M of HNO3 (aq) at 25 degrees celsius identify the relative molar amounts of theses species HNO3- H3O+ OH- NO3- H2O
Friday, February 21, 2014 at 2:51pm by Joe

chemistry
NACL +HNO3 = HCL +NANO3 AGCL + HNO3= NO REACTION With regards from SHABAZ AHMED DAR ( VIVEKANANDA KENDRA VIDYALAYA) BARAGOLAI, ASSAM
Sunday, March 13, 2011 at 9:02pm by shabaz ahmed dar (vkv baragolai)

Molarity
A 15.7mL sample of HNO3 reacts to neutralize 27.7mL of 0.187M KOH solution. What is the molarity of the HNO3 solution? HNO3 + KOH ==> KNO3 + HOH mols KOH = L x M = 0.0277 x 0.187 = ?? mols HNO3 = mols KOH (1 mol reacts with 1 mol). mols HNO3 = L x M You have mols HNO3 and L...
Sunday, February 25, 2007 at 10:40pm by Kellie

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
In a 1.0x10^-6 M solution of HNO3(aq) at 25 degrees C, identify the relative molar amounts of species from most to least. HNO3 H3O+ H2O OH- NO3-
Thursday, February 20, 2014 at 11:12am by Mer

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
millimols NH3 = M x mL = ? mmols NH4Cl = mL x M = ? mmols HNO3 = mL x M = ? Before: Use the Henderson-Hasselalch equation. After: Construct an ICE chart frp, below and add the HNO3. Recalculate using the HH equation. ............NH3 + H^+ ==> HNH4^+ initial..... add HNO3...
Sunday, March 18, 2012 at 3:46pm by DrBob222

Chemistry II
HNO3 + NaOH ==> NaNO3 + HOH Notice ratio acid/base = 1:1 pH 3.78 = (H^+) = (HNO3) = 1.7E-4 (approximate--you should do it more accurately.) 1.7E-4 moles/L x 1.6E4L = about 3 moles = moles HNO3 = moles NaOH needed. M NaOH = moles NaOH/L NaOH. You have M and moles, solve for L.
Monday, October 3, 2011 at 9:37pm by DrBob222

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