A beaker with 105 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.30 mL of a 0.470 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.

Express your answer numerically to two decimal places. Use a minus ( − ) sign if the pH has decreased.

Note: Please provide a professional 4th-year level with a clear explanation or LEAVE the question for someone else to answer!

Hypothetically, if DNA was used as form data storage for digital devices, what are two potential advantages and two potential disadvantages to its use, compared to a standard hard drive?

name the three properties that will be varied in lab to determine how they affect the rate at which solid dissolves into solution

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 30.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C), calculate the final temperature of the solution.

            Ca2+(aq) + 2 F-(aq) → CaF2(s)   ΔH° = -11.5 kJ

30.55°C

If there is additional information about the heat capacity of the calorimeter (58.3 J/°C) in the above questions, how would you approach your answer?

What is the pH when 30 ml of 1M hydrochloric acid is added to 200 mL of distilled water?

please writing hot to solve it .

Consider the titration of a 12.0 mL solution containing 0.200 mol/L acetic acid (CH3COOH, Ka = 1.8 x 10-5 ), with a solution of 0.250 mol/L KOH. (12 points total) i) Determine the pH of the solution when 4.80 mL of KOH has been added.

ii) Determine the pH of the solution when 14.00 mL of KOH has been added.

6. For the complete redox reaction given here, (a) break down each reaction into its half reactions; (b) identify the oxidizing agent; and (c) identify the reducing agent.

3F2 +2AlCl3 →2AlF3 +3Cl2

Answer the following questions:

a) Does an isomer of ethanol have a strong or weak interaction (intermolecular) with the stationary phase in gas chromatography if the isomer have a less retention time than ethanol? Explain.

b) At sea level, the boiling point for ethanol is 78.4 C. If you want to purify ethanol where the altitude is 430 m below sea level, do you think the boiling point be higher or lower than 78.4 C? Explain.

A- a small volume of cold water is used to cool off a cup of coffee that is initially too hot to drink. How many mL of water at 4.0oC must be mixed with 485 mL of hot coffee (95.0oC) so that the resulting combination has a temperature of 70.0oC? Assume that the coffee and water have the same density and specific heat.   

B- A 5.00 cm³ sample of aluminum at room temperature (25.00^oC) was dropped into a 1 L beaker of boiling water (100.00^oC) and allowed to come to equilibrium. How much heat was absorbed by the aluminum cube? The specific heat capacity of aluminum is 0.902 J/g·K and its density is 2.70 g/cm³.

C- When 50.00 g of 0.200 M NaCl (aq) at 24.1^oC is added to 100.0 g of 0.100 M AgNO₃ (aq) at 24.1^oC in a calorimeter, the temperature increases to 25.2oC as AgCl (s) forms. Assuming the specific heat of the solution and products is 4.20 J/g^oC, calculate the number of joules of heat produced in the reaction.

A buffer solution contains 0.430 M NaHCO₃ and 0.284 M Na₂CO₃. Determine the pH change when 0.062 mol HI is added to 1.00 L of the buffer.

pH change=____

Determine the pH of a 0.150 M benzoic acid solution with a  Ka = 6.5 x 10^–5.  

- report the answer in three significant figures

Calculate the expected buffer capacity of the acetate buffer based on the number of moles of CH3CO2H in the buffer. (hint, you know the concentration and volume) In other words, how many moles of NaOH are needed to break the buffer? Does the measured buffer capacity of acetate buffer (20mL) meet your expectations?

pKa = 4.74

target pH= 4.9

[HA]= 2.04x10-2 M [A] = 2.96x10^-2 M

Calculate the mass of sodium acetate (NaC2H3O2) that must be added to make 100 mL of an acetic acid/acetate buffer at pH = 5.0, given that you will use 5.0 mL of 0.50 M acetic acid.

1. Calculate the concentration of acetic acid after 5.0 mL of 0.50 M acetic acid has been diluted to 100.0 mL.

2. Using the Henderson-Hasselbalch equation, calculate the concentration of NaC2H3O2 need in the buffer.

3. Calculate the mass of NaC2H3O2 needed to make 100.0 mL of solution of the concentration you determined in part 2.

4. If you needed a buffer of pH 5.5, would you require more or fewer grams of NaC2H3O2? Why?

PLEASE HELP ME

11.5 mL of a 0.399 M sodium phosphate solution reacts with 19.9 mL of a 0.192 M lead(II) nitrate solution. What mass of precipitate will form?

List 5 reactions to produce Ethyl Bromide and show the mechanisms