Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O. Suppose 2.4 g of hydrobromic acid is mixed with 0.876 g of sodium hydroxide. Calculate the maximum mass of sodium bromide that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.

1.What is the pH at the equivalence point when 0.100 M weak acid HA (Ka = 1.48 x 10 - 4) is titrated with 0.050 M KOH?

2.Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M KCN with 4.33 mL of 0.425 M strong acid HCl. HCN pKa = 9.21

3.Strong bases, NaOH and KOH can not be used as primary standards because of the presence of ______________ A.carbonate B.water C.adsorbed water

please explain each step by step, thank you

PLEASE ANSWER THOROUGHLY AND BREAK DOWN EACH STEP. THANK YOU!!

Characteristics of Chemical Equilibrium

The purpose of this lab is to investigate how changing various factors affect an equilibrium system. This lab consists of four independent activities. Each activity changes a component (concentration, temperature, and pressure) in an equilibrium system. Students observe how the changes affect the equilibrium system and analyze the changes using Le Chatelier’s Principle.

Please explain your answers to the following questions using Le Chatelier’s Principle.

Activity A: Nature of Equilibrium

            HIn (aq)    ↔     H⁺(aq)     +      In^– (aq)        …… (A)

            Colorless                                    Pink

            H⁺(aq)       +     OH^-(aq) →     H₂O (l)

If HCl solution is added to the solution in equilibrium A, would the solution become more pink or less pink?

If NaOH solution is added to the solution, which direction would the equilibrium shift to? Would the color become more pink or less pink when NaOH solution is added to the equilibrium?

Activity B: Effect of Concentration

            Fe³⁺⁽aq)      +        SCN^-(aq)       ↔     FeSCN²⁺(aq) ………   (B)

            yellow                     colorless                 red

            Fe³⁺(aq)       +        H₂PO₄^-(aq)   →     FeH₂PO₄²⁺(aq)

            yellow                    colorless                 colorless

Which direction would the equilibrium shift to if Fe(NO₃)₃ solution is added to the equilibrium B?

Which direction would the equilibrium shift to if Na₃PO₄ is added to the equilibrium B?

Activity C: Effect of Temperature

1. Fe³⁺⁽aq)      +       SCN^-(aq)       ↔     FeSCN²⁺(aq)       is an exothermic reaction.

yellow                 colorless                     red

Would the color of the solution become more red or less red if the temperature is increased? What happens if the temperature is decreased?

2. Co(H₂O)₆²⁺ (aq)    +     4Cl^–(aq)    ↔     CoCl₄^2- (aq)     +    6H₂O (l)

pink                                                               blue

When the solution is heated to boiling, it turns from pink to blue.

Is this reaction endothermic or exothermic?

Bonus: if AgNO₃ is added to the above blue solution, would the solution change color back to pink? If HCl is then added to the solution, would the color change again?

Activity D: Effect of Pressure

2 CO₂(g)    +      H₂O(l)   ↔   CO₂ (aq)   +   H⁺(aq)     +   HCO₃^-(aq)

The reaction forms equilibrium in a large syringe with changeable volume.

Would the solution become more acidic or less acidic when the volume is increased? What happens if the volume is decreased?

Consider a diporitc acid, H₂A, where K_a1 = 8.41E-4 and K_a2 = 2.36E-9. Answer the following questions regarding this solution:


If the initial concentration of the acid is 0.66M, what is the pH of the solution?

What will the concentration of A^2- be at equilibrium?

Indicate how you would carry out each of the following reactions. How would you distinguish between the starting material and product by IR? Your answer should include both disappearance as well as appearance of IR absorptions.

A) 1-methylcyclohexene to trans-2-methylcyclohexanol

B) cyclohexene to cis-1,2-cyclohexandiol

C) 1-hexyne to 2-hexanone

D) 1-hexyne to 1-hexene

E) 3-chloropentane to 2-pentene

Draw the Lewis Dot Structure for the following compounds and then determine

a) the hybridization of the central atom

b) the electron group arrangement

c) the bond angle around the central atom

d) the molecular geometry.

a) H₃O⁺          

b) NO₃^-                

c) O_{3      `}                

d) HCN          

e) CH₃CH₃

A buffer contains 0.11 mol of propionic acid (C2H5COOH) and 0.17 mol of sodium propionate (C2H5COONa) in 1.20 L. What is the pH of this buffer?

What is the pH of the buffer after the addition of 0.02 mol of NaOH?

What is the pH of the buffer after the addition of 0.02 mol of HI?

ANSWER TWO OF THE FOLLOWING QUESTIONS :

A 24.1 mL sample of a 0.353 M aqueous acetic acid solution is titrated with a 0.426 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added?

pH =

A 46.1 mL sample of a 0.455 M aqueous nitrous acid solution is titrated with a 0.292 M aqueous barium hydroxide solution. What is the pH after 22.0mL of base have been added?

pH =

What is the pH at the equivalence point in the titration of a 22.8 mL sample of a 0.439 M aqueous hypochlorous acid solution with a 0.497 M aqueous sodium hydroxide solution?

pH =

A heat lamp produces 22.0 watts of power at a wavelength of 6.8 μm . How many photons are emitted per second? (1 watt = 1 J/s). The answer needs to be in s^-1

Calculate the pH at the stoichiometric point when 25 mL of 0.089M formic acid is titrated with 0.33 M NaOH.

Calculate the pH at the stoichiometric point when 25 mL of 0.096 M pyridine is titrated with 0.31 M HCl.

Calculate the pH at the stoichiometric point when 25 mL of 0.093 M nitric acid is titrated with 0.34 M NaOH.

Chapter 8: Electron Configurations and Periodicity Complete for a thumbs up!

a. Write the electronic configuration and draw the orbital diagram of iron.

b. Create a table summarizing the group traits of elements.

c. Explain why Hund's rule is incredibly important. Use examples or images to help back up your explanation

d. In the science field, chemists often use NMR for confirmation of the structure of newly synthesized drugs. This is what MRIs do to humans at hospitals. Please explain what these machines are doing at an atomic level. Use your own words, and try your best to relate it to the material covered in this chapter

Given the pH and absorbance of a solution. What equation would i use to find the

1.equilibrium concentration of the base? 2. equilibrium concentration of the acid?

Fischer Synthesis of Isopentyl Acetate

Data:

Inital Amounts: 1mL Isopentyl alcohol + 1.5mL glacial acetic acid

amount of product collected = 1.727 g

Question: Was the reaction successful? What was the actual yield? (You may need to do some unit conversions for this) Please explain as well