In a reaction, aqueous NaOH is titrated against sulfuric acid solution, H2SO4, according to the equation:

2 NaOH (aq) + H2SO4 (aq) --> Na2SO4 (aq) + 2H2O (l)

If 18.62 ml of sulfuric acid are neutralized with 25.00 mL of 0.100 M NaOH, what is its molar concentration (Molarity, M) of sulfuric acid solution?

Hey guys,

So I am doing a presentation on the element Gold, Au. Now I could go look up the information online but I am really running out of time here, could someone provide me with as much information as you can on the elemnt gold(NOTE NOT PLAGIARIZED). Please cite everything and just hook me up with as many paragraphs and information on gold as you can. I will downrate you if you just do a lazy copy paste from google so please be cautius. If this is too much then just ignore this question. BTW even if you can't write paragraphs about gold, try to atleast give me some ideas and questions about the element so that I can answer and finish this powerpoint. THANK YOU!

Explain why the mutation of Asp-52 to Asn-52 decreases enzyme activity of lysozymes by 10,000 fold.

Solution	Absorbance	[Fe(SCN)2+]eq
B-1	0.060	1.4*10-5
B-2	0.151	3.8*10-5
B-3	0.323	8.07*10-5
B-4	0.381	9.5*10-5
B-5	0.427	1.06*10-4

Solution	Vol of 0.002 M Fe3+	Volume of 0.002 M SCN-	Volume of H2O
B-1	5.0 mL	1.0 mL	5.0 mL
B-2	5.0 mL	2.0 mL	4.0 mL
B-3	5.0 mL	3.0 mL	3.0 mL
B-4	5.0 mL	4.0 mL	2.0 mL
B-5	5.0 mL	5.0 mL	1.0 mL

2. Determine the equilibium concentration of each of the reactants and products in Solution B-1 using the table provided below (ICE table). Fill in all blank values

	[Fe3+]	[SCN-]	[Fe(SCN)2+]
Initial Concentration
Change in Equilibrium
Equilibrium Concentration

3.Determine the equilibium concentration of each of the reactants and products in Solution B-2 using the table provided below (ICE table). Fill in all blank values

	[Fe3+]	[SCN-]	[Fe(SCN)2+]
Initial Concentration
Change in Concentration
Equilibrium Concentration

4.Determine the equilibium concentration of each of the reactants and products in Solution B-3 using the table provided below (ICE table). Fill in all blank values

	[Fe3+]	[SCN-]	[Fe(SCN)2+]
Initial Concentration
Change in Concentration
Equilibrium Concentration

5. Determine the equilibium concentration of each of the reactants and products in Solution B-4 using the table provided below (ICE table). Fill in all blank values

	[Fe3+]	[SCN-]	[Fe(SCN)2+]
Initial Concentration
Change in Equilibrium
Equilibrium Concentration

6.Determine the equilibium concentration of each of the reactants and products in Solution B-5 using the table provided below (ICE table). Fill in all blank values

	[Fe3+]	[SCN-]	[Fe(SCN)2+
Initial Concentration
Change in Equilibrium
Equilibrium Concentration

I have no idea how to do problems 2-6. Could someone please help me. Your help is always greatly appreciated! Thank you in advance.

combining selected ion monitoring (SIM) with isotope dilution in electron ionization mass spectrometry allows:

In an experiment similar to this one, the solubility of potassium hydrogen oxalate (KHC2O4, molar mass= 128.13 g mol) is determined. A 5.0 10^-2 M aqueous solution of KCI is saturated with potassium hydrogen oxalate. The following equilibrium results: KHC2O4(s)-----K^+ + HC2O4^-

Following saturation, the solution is filtered. Portions of the filtered saturated solution are titrated with 0.1172M NaOH solution.

The following date are obtained:

Volume of saturated KHC2O4 Solution Titrated, mL Determination #1 25.2 Determination #2 29.1

Volume of NaOH solution used, mL ---------------------Determination #1 36.88 Determination #2 41.81

Temperature of saturated solution, C-------------------- Determination #1 20.1 Determination #2 20.1

Calculate the following:

number of moles off NaOH needed, mol _______________________For both determinations

number of moles of HC2O4 ^- titrated, mol______________________For both determinations

[HC2O4^-] sat. sol'n_______________________________________For both determinations

[K^+]initial______________________________________________For both determinations

[K^+]from dissolved KHC2O4________________________________For both determinations

[K^+] sat. sol'n___________________________________________For both determinations

Ksp___________________________________________________For both determinations

average Ksp

solubility of KHC2O3 in 5.0 x 10^-2M KCI, mol L___________________for both determinations

Average solubility of KHC2O4 in 5.0 x 10^-2 KCI, mol L

solubility of KHC2O4 in 5.0 x 10^-2 M KCI, g per 100 mL

Use the following cell to answer the questions:

Cr / Cr3+ (1.00 M) // Ni2+ (1.00 M) / Ni.

a) How many milligrams of Ni would be plated on the cathode if a current of 0.39 A is drawn for 2.0 hrs?

b) What is [Cr3+] when [Ni2+] has dropped to 10-4 M?

c) What is the cell potential at the conditions described in Part b?

Table of standard reduction potentials: http://www.chemeddl.org/services/moodle/media/QBank/GenChem/Tables/EStandardTable.htm

Nuclear binding energy

Part D

Calculate the mass defect of the helium nucleus 52He. The mass of neutral 52He is given by MHe=5.012225amu.

Express your answer in atomic mass units to four significant figures.

	amu

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Part E

Calculate the binding energy E of the helium nucleus 52He (1eV=1.602×10−19J).

Express your answer in millions of electron volts to four significant figures.

E =		MeV

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Part F

Calculate the binding energy per nucleon of the helium nucleus 52He.

Express your answer in millions of electron volts to four significant figures.

	MeV

What is the concentration of hydroxide ions after 50.0 mL of 0.250 M NaOH is added to 120 mL of 0.200 M Na2SO4?

What is the concentration of hydroxide ions after 50.0 mL of 0.250 M NaOH is added to 120 mL of 0.200 M Sr(OH)2?

What is the advantage of using an internal standard in a gas chromatography experiment?

How many milliliters of 8.00 M KOH must be added to neutralize the following solution? a mixture of 0.240 M LiOH (25.0 mL) and 0.200 M HBr (75.0 mL)

Write balanced net ionic equation for the following reaction:

HBr(aq)+Ca(OH)2(aq)→?

Classify each of the following reactions as a precipitation, acid-base neutralization, or oxidation-reduction.

a.) Hg(NO3)2(aq)+2NaI(aq) → 2NaNO3(aq)+HgI2(s)

b.) H3PO4(aq)+3KOH(aq) → K3PO4(aq)+3H2O(l)

1. Write a net ionic equation for the following reaction
Na2CrO4(aq)+Pb(NO3)2(aq)→?

2. Write a net ionic equation for the following reaction
AgClO4(aq)+CaBr2(aq)→?

3. Write a net ionic equation for the following reaction
ZnCl2(aq)+K2CO3(aq)→?

4. What is the molecular formula of salicylic acid?

5. Assume that you have 1.50 mol of H2 and 3.50 mol of N2. How many grams of ammonia (NH3)can you make, and how many grams of which reactant will be left over?
3H2+N2→2NH3

mNH3 =

mH2 =

mN2 =

6. What is the molarity of an HNO3 solution if 69.0 mL is needed to react with 25.0 mL of 0.150 MKOH solution? The equation is
HNO3(aq)+KOH(aq)→KNO3(aq)+H2O(l)

7. What mass of carbon dioxide is produced from the complete combustion of 1.10×10⁻³ g of methane?

8. What mass of water is produced from the complete combustion of 1.10×10⁻³ g of methane?

9. What mass of oxygen is needed for the complete combustion of 1.10×10⁻³ g of methane?

Can you please show me how to do these problems? Thank You So Much!

When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is

CH4(g)+O2(g)→CO2(g)+H2O(g)

This type of reaction is referred to as a complete combustion reaction.

Part B-What mass of carbon dioxide is produced from the complete combustion of 3.00×10⁻³ g of methane?

Part C-What mass of water is produced from the complete combustion of 3.00×10⁻³ g of methane?

Part D- What mass of oxygen is needed for the complete combustion of 3.00×10⁻³ g of methane?

Balance the following reaction in acidic conditions. If a 74.8 mL sample of a solution of H2C2O4 (aq) requires 27.5 mL of a 0.037 M KMnO4 solution for a complete reaction, what is the concentration of H2C2O4 in the original solution?

MnO4- (aq) + H2C2O4(aq) -> Mn2+(aq) + CO2(g)

Answer True or False for the following statement: a)In the following chemical reaction, CaO is the reducing agent. 2Ca(s) + O2 (g) → 2CaO (s) b)In the following chemical reaction, H2O is the reducing agent. 4Fe(OH)2 (s) + O2 (g) + 2H2O (l) → 2Fe2O3.3H2O (s)

Long and detailed theory behind HPLC. An introduction to HPLC and how the technique/instrument work and why one would want to measure the concentration of caffeine in a sample is essential.