How does indicator works and how does one select an indicator?

What is titration and why titrations are useful?

1. Explain how the pH of the solution is changing using the titration curve.
2. Describe the process in which you would titrate a weak acid with a strong base. Include an image of a titration curve.

3. Explain the titration curve of a polyprotic acid.

4. Difference between endpoint and equivalence point?

Balance each of the following redox reactions occurring in acidic solution.

PbO₂(s) + I^?(aq) ? Pb²⁺(aq) + I₂(s)

SO₃^2?(aq) + MnO₄^?(aq) ? SO₄^2?(aq) + Mn²⁺(aq)

S₂O₃^2?(aq) + Cl₂(g) ? SO₄^2?(aq) + Cl^?(aq)

This is a two part question. Calculate either [H3O+] or [OH−] for each of the solutions at 25 °C.

Solution A: [OH−]= 2.91×10−7 M Solution A: [H3O+]= M

Solution B: [H3O+]=9.81×10−9 M   Solution B: [OH−]= M

Solution C: [H3O+]=0.000669 M Solution C: [OH−]= M

Which of these solutions are basic at 25 °C? (You are able to pick more than one option). Solution C, Solution A, and Solution B are the three options.

Solution C: [H3O+]= 0.000669 M

Solution A: [OH−]= 2.91×10−7 M

Solution B: [H3O+]= 9.81×10−9 M

What is theoretical yield

Find the concentration of all species in solution for a 0.25 M aqueous solution of H₂CO₃.         Hint (which would NOT be given for an exam): all species includes H₂CO₃, HCO₃^-, CO₃^2-, H₃O⁺, AND OH^-.

A 1.912-g sample of calcium chloride is decomposed into its constituent elements and found to contain 0.690 g Ca and 1.222 g Cl. Calculate the mass percent composition of Ca and Cl in calcium chloride.

4. 62.4 mL of 0.39 M NaCl solution was added to 26.8 mL of 058 M Pb(NO3)2 solution. a. Write the full balanced reaction, the molecular ionic equation and the net ionic equation.
b. What is the precipitate? c. How many grams of the precipitate can be made

15. What does the term quantized energy mean?

How many quantum numbers are known with respect to atomic orbitals?

Name them and provide their key properties

What are the freezing point and boiling point of a solution prepared by dissolving 18.6g of CaCl₂ in 200.0g of water? (k_f = -1.86�/m and k_b= 0.512�/m)?

Find the pH of each of the following aqueous solutions.

            a.         0.25 M CH₃COOH

            b.         0.25 M HNO₃

            c.          0,25 M KCH₃COO

d.         0.25 M KOH

            e.         0.25 M NH₃

            f.          0.25 M NH₄Cl

For each of the following strong base solutions,determine [OH], [H3O+], pH, pOH:

0.18M NaOH

1.7*10^-3m Ca(OH)2

5.0*10^-4M Sr(OH)2

8.8*10^-5M KOH

1) Which of the following can behave as Bronsted-Lowry bases in aqueous solution?
HNO2
H2SO3
Ca2+
I-
None of the Above

2) Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

Ba(OH)₂

KOH

CN^-

NH₃

None of the Above

1) Calculate the ∆H value for the following unbalanced reaction using equations 1 and 2.    C (s) + H ₂ O (g) → CO ₂ (g) + H ₂ (g)

Equation 1: C _(s) + O _2(g) → CO _{2 (g)}                 ∆H = –304 kJ

Equation 2: H _{2 (g)} + O ₂ (g) → H ₂ O _(g) ∆H = –242 kJ

2) Given 0.150 L of nitrous oxide at 25 °C and 749 mmHg pressure, calculate the number of N 2 O molecules

3) If 45.5 mL of 0.150 M sodium sulfate solution reacts with 50.0 mL of 0.175 M aqueous barium nitrate

4) What is absolute zero? How do gas particles behave at this temperature? List any four ideal gas

5) What is the [OH - ] of a solution that has a [H O + ] of 5.0 × 10 -2 M? Is this solution acidic, basic or neutral?