A 300.0 mL buffer solution is 0.230 M in acetic acid and 0.230 M in sodium acetate.

Part A: What is the initial pH of this solution?

Part B: What is the pH after addition of 0.0050 mol of HCl?

Part C: What is the pH after addition of 0.0050 mol of NaOH?

Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). A list of ionization constants can be found here.

A 5.193 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 9.255 grams of CO₂ and 3.790grams of H₂O are produced.

In a separate experiment, the molar mass is found to be 74.08 g/mol. Determine the empirical formula and the molecular formula of the organic compound.

Enter the elements in the order C, H, O

Answer the questions completely with complete calculations.

1. Balance the following equation & fill in the state of the chemicals.

a. Fe2 (SO4)3 (aq) + NH3 (aq) + H2O (l) --> Fe (OH)3 ( ) + (NH4)2SO4 ( )

2. How many atoms of oxygen are present in 1.75 g sample of Fe2 (SO4)3?

3. Calculate the percentage of Cl by mass in PCl5

4. Predict whether each of the following ionic compounds is likely to be water soluble.

KCl _____; MgCO3 ____

Fe2O3 ____; Cu(NO3)2 _____

In which compound will the bulb be lit most brightly? why?

5. What is the oxidation number of element in BrO2-, BrO3- & BrO4-, Br2, Br-?

6. In the reaction 4 NH3 (g) + 5 O2 (g) --> 4 NO (g) + 6 H2O (l)

750 g NH3 is mixed with 750 g of O2.

a. what is the amount of NO produced in this reaction?

b. which is the limiting reagent?

c. How much of the excess reagent remains?

d. The actual yield of NO obtained was 400g. What is the % yield of NO?

7. A compound of 49.4% K, 20.3% S, and 30.3% O by mass. What is empirical formula of the compound?

8. How many grams of a sample of NaNO3 should be dissolved in a 150.0 mL of water to give a 0.22 M solution?

9. A certain alcohol contains only three elements C, H & O. Combustion of 50.00 g sample of the alcohol produced 95.50 g of CO2 and 58.70 g of H2O. What is the empirical formula of the alcohol?

The dibasic compound B (pKb1 5.00, pKb2 9.00) was titrated with 0.5 M HCl. The initial solution of B was 0.0500 M and had a volume of 50.0 mL. Find the pH at the following volumes of acid added Va = 0, 1, 5, 9, 10, 11, 15, 19, 20, and 22 mL.

Part A: What mass of water is produced from the complete combustion of 5.90×10−3 g of methane?

Part B: What mass of oxygen is needed for the complete combustion of 5.90×10−3 g of methane?

1. a.) What is the pH of a solution created by combining 1.27 mole of HOBr and 0.43 mole NaOH in a 1.00L solution? Ka HOBr = 2.5 x 10-9

b.)What is the pH of a buffer made by combining 0.98 moles HOBr with 0.67 moles NaOBr in a 100.00mL solution? Ka HOBr = 2.5 x 10-9

To prepare 0.250 L of 0.100 M aqueous NaCl (58.4 g/mol), one may

1. Does the pH increase, decrease or remain the same on the addition of the of the following?

a.) LiF to an HF solution b.)KI to an HI solution c.)NH4Cl to an NH3 solution d.) HBr to an CH3COO-/CH3COOH (acetic acid/acetate buffer) solution

2. Which of the following (select all that apply) gives a buffer solution when equal volumes of the two solutions are mixed?

A 340.0 −mL buffer solution is 0.140 M in HF and 0.140 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? And, If the same volume of the buffer was 0.370 M in HF and 0.370 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00? Please show all steps. Thank you

13.Explain each term in the Van Deempter Equation (Below). What major advantage is gained through open tubular GC in reference to this equation?

At a certain temperature, 0.920 mol of SO3 is placed in a 4.00-L container. 2SO3(g) <===>2SO2(g) + O2(g) At equilibrium, 0.130 mol of O2 is present. Calculate Kc.

Intro to the problem:

To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH.

A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO−. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH3COO).

Buffers work because the conjugate acid-base pair work together to neutralize the addition of H+ or OH− ions. Thus, for example, if H+ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H+ with the conjugate base:

H++CH3COO−→CH3COOH

Similarly, any added OH− ions will be neutralized by a reaction with the conjugate acid:

OH−+CH3COOH→CH3COO−+H2O

This buffer system is described by the Henderson-Hasselbalch equation

pH=pKa+log[conjugate base][conjugate acid]    

Part A

A beaker with 1.80×10² 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 5.60 mL of a 0.330 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.

3) for one resonance structure of a nitrate(NO3-) provide the:
a) Lewis structure

b) formal charge on each atom

c)name of the electro pair(electron domain) geometry

d) hybridization of the central atom

e)name of the molecular geometry (shape)

When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. How many grams of calcium chloride will be produced when 25.0 g of calcium carbonate are combined with 14.0 g of hydrochloric acid?Which reactant is in excess and how many grams of this reactant will remain after the reaction is complete?

I found that there is 21.01 Grams of CaCl2