Homework Answers
Add Answer to:
final molarity of ammonium
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and...
urgent!!! The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4,...
urgent!!!
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4, MM = 98.00 g/mol) proceeds according to the following balanced eqation: 3NH4OH(aq) + H3PO4(aq) ->3H20(1) + (NH4)3PO4(aq) What is the final molarity of the ammonium ion (NH4+, MM = 18.05 g/mol) when 25.0 mL of 1.20 molar ammonium hydroxide is reacted with 25.0 mL of 2.00 molar phosphoric acid?
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You...
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You have 80 mL of a 0.5 M NHOH solution and 40 mL of a 7.5% (w/v) NH4OH solution. What volume of 7.5% NHOH and water needs to be added to the 80 mL of 0.5 M NH4OH solution to make up 200 mL of 0.4 M NH4OH? Molar mass of NH4OH 35.04 g/mol % (weight / volume) means mass (in g) in volume (100...
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L...
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH ----> H2O (l) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L...
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH ----> H2O (l) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L...
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH --> H2O (1) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00...
1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00 M hydrochloric acid with 100 mL of 1.20 M sodium hydroxide. The initial temperature was 22.88 °C and the final temperature was 29.39 °C. Calculate the calorimeter constant for the reaction. HCl (aq) + NaOH (aq) NaCl (aq) + H2O (∆H°rxn = -58.3 kJ/mol) 2. The same calorimeter was used for the dissolution of 8.86 g sample of lithium chloride in 100.0 mL of...
Five grams of citric acid (MM=180.0 g/mol) are dissolved in 100.0 g water. the resulting solution...
Five grams of citric acid (MM=180.0 g/mol) are dissolved in 100.0 g water. the resulting solution reacts with 65.3 mL of strontium hydroxide solution. the balanced net ionic equation for the reaction is H3C5H5O7 (aq) +3OH^-(aq)-->C5H5O7^3- (aq) + 3H2O what is the molarity of the strontium hydroxide solution? the answer is .638 in my answer key but I don't know how to get it. thanks
Worksheet 2 2. Calculate the concentration of each of the following solutions. Determine the molarity (mol/L)...
Worksheet 2 2. Calculate the concentration of each of the following solutions. Determine the molarity (mol/L) of a solution made by diluting 5.880 g of barium chloride to a final volume of 525.0 mL a. b. What is the molarity of a solution that dilutes 12.50 mL of 6.00 M HCI (hydrochloric acid) to a final volume of 1.50 L? If you combine 1.55 g of NH CI (ammonium chloride) with 2.38 g of CaCl, (calcium chlo- ride) and dilute...
20. Identify the neutralization reaction. Classify all of the reactions shown below. a) CH4 (g) +...
20. Identify the neutralization reaction. Classify all of the reactions shown below. a) CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) b) MgBr2 (aq) + Cl2 (g) → MgCl2 (aq) + Br2 (l) c) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) d) BaCl2 (aq) + 2 AgNO3 (aq) → 2 AgCl (s) + Ba(NO3)2 (aq) 23) Calculate the mass and the number of the hydroxide ions in Ca(OH)2 required to react...
15. The mixing of which pair of reactants will result in a precipitation reaction? CsI(aq)...
15. The mixing of which pair of reactants will result in a precipitation reaction? CsI(aq) + NaOH(aq) HCl(aq) + Ca(OH)2(aq) K2SO4(aq) + Hg2(NO3)2(aq) NaNO3(aq) + NH4Cl(aq) 16. Which of the following is a precipitation reaction? Zn(s) + 2 AgNO3(aq) 2 Ag(s) + Zn(NO3)2(aq) NaCl(aq) + LiI(aq) NaI(aq) + LiCl(aq) 2 KI(aq) + Hg2(NO3)2(aq) Hg2I2(s) + 2 KNO3(aq) HI(aq) + NaOH(aq) NaI(aq) + H2O(l) None of these are precipitation reactions. 17. Which...
urgent!!!
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4, MM = 98.00 g/mol) proceeds according to the following balanced eqation: 3NH4OH(aq) + H3PO4(aq) ->3H20(1) + (NH4)3PO4(aq) What is the final molarity of the ammonium ion (NH4+, MM = 18.05 g/mol) when 25.0 mL of 1.20 molar ammonium hydroxide is reacted with 25.0 mL of 2.00 molar phosphoric acid?
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You have 80 mL of a 0.5 M NHOH solution and 40 mL of a 7.5% (w/v) NH4OH solution. What volume of 7.5% NHOH and water needs to be added to the 80 mL of 0.5 M NH4OH solution to make up 200 mL of 0.4 M NH4OH? Molar mass of NH4OH 35.04 g/mol % (weight / volume) means mass (in g) in volume (100...
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH --> H2O (1) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
Worksheet 2 2. Calculate the concentration of each of the following solutions. Determine the molarity (mol/L) of a solution made by diluting 5.880 g of barium chloride to a final volume of 525.0 mL a. b. What is the molarity of a solution that dilutes 12.50 mL of 6.00 M HCI (hydrochloric acid) to a final volume of 1.50 L? If you combine 1.55 g of NH CI (ammonium chloride) with 2.38 g of CaCl, (calcium chlo- ride) and dilute...
Most questions answered within 3 hours.
-
Where is the error in this code sequence?
String s1 = "Hello";
String s2 = "ello";...
asked 10 months ago -
Financial data for Joel de Paris, Inc., for last year
follow:
Joel de Paris, Inc.
Balance...
asked 10 months ago -
Consider this reaction:
Al2(SO4)3 (aq)+ BaCl3
(aq) Al2Cl6 (aq)- +
3BaSO4(s) . What is the...
asked 10 months ago -
Suppose that Savneet is considering increasing her
recent random sample from 20 car rentals to 40...
asked 10 months ago -
Trucks arrive at an unloading terminal at an average rate of 120
per hour.
Trucks arrive...
asked 10 months ago -
Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
asked 10 months ago -
A facilities manager at a university reads in a research report
that the mean amount of...
asked 10 months ago -
When the CuSO4 is rehydrated by adding water to the anhydrous
compound, is this an endothermic...
asked 10 months ago -
A ray of sunlight is passing from diamond into crown glass; the
angle of incidence is...
asked 10 months ago -
A block of mass 0.249 kg is placed on top of a light, vertical
spring of...
asked 10 months ago -
how do the kidneys compensate in the presences of acidosis
a) trigger hyperventilate
b) reserve acid...
asked 10 months ago -
Question 501 pts
The rental rate of capital to the firm increases. Which of the
following...
asked 10 months ago