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Acids and Bases

Chemistry

1. Given the following table of Ksp values, determine which compound listed has the smallest solubility. compound Ksp CdCO3 5.2 x 10-12 Cd(OH)2 2.5 x 10-14 AgI 8.3 x 10-17

Lab experiment - six prepared solutions

1) This is the scenario: there are six prepared solutions, but the labels are not on the bottles. What are the the solutions in the bottle. The six possible solutions are silver nitrate, barium chloride, copper (II) nitrate, copper(II) sulfate, sodium carbonate, and hydrochloric acid. The results were found by mixing the each so

Molarity, Mole, Dilution

See the attached file. 1. A sample of concetrated nitric acid has density of 1.41g/ml and contains 70% HNO3, by mass. a. What mass of HNO3 is present per litre of solution?(in g/l) b. What is the molarity of the solution? 2. Calculate each of the following quantities. a. molarity of a solution prepared by diluting 3

Salt formation from neutralization of reaction.

What is the name of the salt formed by the complete neutralization of sulfuric acid with lithium hydroxide? Choices: 1. hydrogen sulfite 2. lithium sulfate 3. lithium hydride 4. lithium sulfide

Acidity and Basicity of Boric Acid

Boric acid, H3BO3, is found in some laundry detergents, antimicrobials, and pesticides. With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work) 1. Write the equation: 2. What is the pH of the solution before titration begin

Solutions to General Chemistry Questions

Which ion(s) is/are spectator ions in the formation of a precipitate of AgBr via combining aqueous solutions of CoBr2 and AgNO3? a. Co2+ and Ag+ b. Co2+ and NO3- c. NO3- and Br- d. NO3- e. Br- Which of the following is an exchange reaction? a. 2SO(g) + O2(g) ---> 2SO2(g) b. CaCO3(s) ---> CaO(s) + CO2(g) c. F

Calculate the pH

Calculate the pH upon diluting 2ml of 2 N HCL to a final volume of 100 ml? Calcuate the pH upon addition of 0.0075 mole of solid NaOH to 100 ml of a 0.1 M solution of acetic acid (pKa=4.7)? If equal molar amounts of Na2HPO4 and NaJpo4 are mixed in water, calcuate the resulting pH. The pKas of phosphoric acid are 2.1, 7.2,

pH of a Mixed Buffer Solution

A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?

Balancing Equations with Calcium Phosphate and Water

Please can you help me, I need to find balanced chemical equations for: a) The reaction of calcium phosphide and water to produce phosphine and calcium hydroxide; b) The oxide formed when phosphorus burns in air, dissolves in water to give a solution of phosphoric acid (H3PO4).

Using Water and Calcium Phosphide to produce phosphine

I have a selection of apparatus and materials that I could use to prepare a gas jar of dry phosphine. I have the following pieces of apparatus to use:- Wash bottle Polythene connectors Dropping funnel with rubber stopper Bent glass tube Filter funnel with paper U-tube Porcelain boat Gas jar Round bottomed flask w

Reduction Potential

Observations: 1) A reacts spontaneously with 1mol/L BNO3, 1mol/L D(NO3)2 and dilute sulfuric acid.A does not react with 1mol/L C(NO3)2. 2) B does not react with any of the 1mol/L solutions above or the dilute sulfuric acid. 3) C reacts spontaneously with dilute sulfuric acid and with 1mol/L solutions of all the other metallic

Diprotic acid with ka1 and ka2

A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 + 2.5E10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHa? What is pKa of the acid component? I don't understand this problem at all! I know that a diprotic substance has something i

Buffer NH3 and NH4Cl

I am really having problems with this problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer. The first part was fair enough, I got 9.35 pH, which is correct. The set up of the second part is tripping me up, I ca

Molarity, electron configuration, and concentration

Question 31 What is the molarity of a solution in which 26.0 grams of BaCl2 (molar mass = 208.2 g/mol) are dissolved in enough water to make 450.0 mL of solution? 0.278 M 0.617 M 1.00 M 3.41 M Question 32 Which element has the following electron configuration? 1s22s22p63s2 Na Mg

Calculating acid dissociation constant

A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 = 2.5E-6. In order to make up a buffer solution of pH 5.8, which combination would you choose, NaHA/H2A or Na2A/NaHA? I know the solution is Na2A/NaHA, but I am not sure why. What is the pKa of the acid component?

NaOH to prepare 576 ml of a solution

How much NaOH is needed to prepare 576 mL of solution with a pH 10? Is it possible to calculate concentration of a solution, OH- concentration, and H+ concentration from just a pH given (no specific base or acid)? Is the concentration of a solution the same as the concentration of [OH-] or [H+]?

Chemical quantities

I need the exact steps that are involved in solving each of these problems and how to arrive at the answers step by step so I can grasp the concept clearly. Thanks. It is very important that I see each step. 1. The gaseous hydrocarbon acetylene, C2H2, is used in welders torches because of the large amount of heat released w

Acidity and Undissociated Acid

A weak acid has a pKa of 3.654. If the solution pH is 3.741, what percentage of the acid is undissociated? A weak acid has a pKa of 5.857. Calculate the pH of a solution in which the ratio of the concentrations of acid anion to undissociated anion ([A-]/[HA]) equals 7.555.

Chemical equations- the Ka and Henderson Hasselbalch equation

Please help, I'm really stuck on the following:- A weak acid has a PKa of 7.713. Calculate the pH of a solution in which the ratio of the concentrations of undissociated acid to acid anion ([HA]/[A-]) equals 8.441 also Calculate the PKa of a weak acid given the information that a 0.652 M solution has a pH of 2.882

Oxidation and reduction problems

1) When iron is oxidized in the presence of nitric acid, three products are formed: iron(III) nitrate, nitrogen dioxide and water. Write and balance the equation for this reaction. Then calculate how many grams of water are formed if 500 grams of iron are reacted with 500 grams of nitric acid. 2) When iron is oxidized in th

Aqueous Solutions

The only possible ions in an aqueous solution are ion, barium, carbonate, chloride and nitrate. The following are observed: i) the original solution contains only dissolved species. ii) adding silver ion to the solution produces no precipitates. iii) adding sulfate ion to the original solution produces a white precipitate

Equilibrium no longer exists - reaction of opening a soft drink bottle

14. In a normal bottle of Coca Cola before it is opened, the following equilibrium exists: H2C03 <=> H+ +HCO3-; Ka = 4.2 x 1 O-7 Once the bottle is opened, this equilibrium no longer exists. Explain what happens, and write a new equilibrium expression showing what happens. I'll give you a hint; there is more than one equil

Equilibrium; Ionization; Concentration

Please see the attachment for complete information. 15. Into a 5.0 liter flask was placed 35.7 g of PCI5 . The flask and contents were heated to 250 0 C, and then held at temperature until the following equilibrium was established: PcI5 (g)< > Pc13 (g) + Cl2 (g) It was then shown by analysis that 875 g of Cl2 was pesent

Stoichiometric Problem

Brass is an alloy of copper and zinc.When ground into a fine powder,then added to hydrochloric acid solution,a single replacement reaction occurs with one of the metals.A soluble salt and hydrogen gas are produced. A)The balnce equation for the reaction that occurs? B)If a 60.0 g sample of the alloy contained enough of the m

Solutions/Acids/Bases

What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1 liter of solution buffered at Ph of 3.55?

Acid-Base Reaction Problem

An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 and pH is 4.20. a. Calculate the concentration of C6H5NH3+ in this buffer solution. b. Calculate the Ph after 4.0 grams of NaOH(s) is added to 1.0 L of this solution. Neglect any volume change.