What are the units for molarity? Rearrange the molarity equation to solve for volume

question 1

The Friedel-Crafts reaction to form BHA forms both isomers equally while the BHT

synthesis only forms on regioisomer (where the t-Bu are ortho to the alcohol). Why is the

selectivity for one regioisomer so much higher in the reaction to form BHT?

explain ir data for 7-Methoxy-1H-indol-6-yl propiolate

IR
(KBr): 3392 (NH), 3259 (C≡CH), 2941, 2810, 2123 (C≡C),
1732 (C═O), (1600, 1500, 1338, 1242, 1200, 1057, 750 cm1)==== specialy

Calculate the concentrations of all species contained in 0.15 M solution of carbonic acid at 25 degrees celsius. ka1= 4.2 x10^-7, ka2= 4.8 x 10^-11 .

The number of different bond angles for PBr2F3 with Br’s axial and equatorial is?

9) A 12.39 kg sample of phosphorus reacts with 52.54 kg of chlorine to form only phosphorus trichloride (PCl3).

a) If it is the only product, what mass of PCl3 is formed?

b) Assuming ideal behavior, calculate the stoichiometric volume of chlorine gas needed at 1.1 atm and 25 °C. 4

c) Calculate the stoichiometric mass of chlorine required.

d) In a similar process, the chlorine is introduced to the reactor in the form of a carbon tetrachloride solution. What volume of a 4.5 M solution is required to deliver for the stoichiometric amount of chlorine?

What is the pH and the equilibrium concentration of PO₄^3- in a 0.511 M solution of H₃PO₄(aq)? Ka1=7.5*10^-3, Ka2=6.2*10^-8, Ka3=4.8*10^-13

0.5 L of a buffer solution contains 0.44 M acetic acid and 0.44 M NaCH3COO, and has a pH of 4.74. What will the pH be if 0.20 mol of HCL is added to the solution?

Learning Goal:

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]   

A beaker with 125mL 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 5.00mL of a 0.380M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.

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

A buffer solution is prepared by dissolving 1.50 g each of sodium benzoate, C6H5COONa, and benzoic acid, C6H5COOH (Ka = 6.45 × 10-5), in 150.0 mL of solution. The molar mass of benzoic acid is 122.12 g/mol and that of sodium benzoate is 144.10 g/mol.

a) What is the pH of this buffer solution?

b) Which buffer component must be added to change the pH to 4.00? What mass of that component is required?

c) What volume of 2.0 M NaOH or 2.0 M HCl must be added to the original buffer in part a to change the pH to 4.00?

The vapor pressure of solid benzene is 299 Pa at -30ºC and 3270 Pa at 0ºC. The vapor pressure of liquid benzene is 6170 Pa at 10ºC, and 15,800 Pa at 30ºC. (a) Calculate the triple point of benzene (temperature and pressure at which solid, liquid, and vapor all coexist). This is obtained by using the Clausius-Clapeyron equation first to determine ∆vapH for the solid and the liquid, and then to give equations for the curves defining the solid-vapor equilibrium and the liquidvapor equilibrium, and solving both the latter equations simultaneously. (b) Calculate the enthalpy of fusion at the triple point, ∆fusH = Hliq – Hsol.

If 91.0g of oxalic acid and 79.0g of methanol react to form 89.0 g of dimethyl oxalate, what is the percent yield?

When you titrate 100 mL of 0.10 M HF with 0.10 M KOH

a) When will this titration reach the equivalence point?

b) Calculate pH when you add 5 mL of KOH.

c) Calculate pH when you add 50 mL of KOH.

d) Calculate pH at the equivalence point.

e) Calculate pH when you add 101 mL of KOH.

(show each step)

Calculate the pH of a buffer solution after the addition of 20.0 mL of 0.200 M NaOH to 80.0 mL of 0.0500 M HC3H5O2 and 0.0250 M NaC3H5O2. (Ka = 1.4 x 10^-5)

Your family is in the business of processing iron from iron ore and after taking Chemistry, you want to help the family business with this knowledge.

Your family business just received a 4000 lb truck load of iron ore from a new customer. You were provided with following background information:

-The iron in the ore has been reduced to Fe²⁺ before redox titration.

-The oxidizing agent used is a standardized 0.086M potassium per manganate (KMnO₄).

-A solution of 1.00 g iron ore required 25.00 mL of 0.086M KMnO₄to reach end point.

-The yield of iron from the iron ore in the entire process is 80%.

What is the Theoretical and Actual Yield from the truck load?