The pKa of the conjugate acid of sodium hydride (NaH) is about 35, the pKa of sodium hydroxide (NaOH) is about 16, and the pKa of the conjugate acid of sodium bicarbonate (NaHCO_3) is about 6.4. What is the mildest base that can deprotonate the molecule below? Draw the structure of the molecule below after it is treated with 2 equivalents of ...

Select all of the correct statements. pKa=50 pKa=19.3 (i) Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation.. SHOW MORE v Butane is more acidic than acetone Acetone is more acidic than butane c Butane can be deprotonated by NaOH

Calculation of pH from Molar Concentrations What is the pH of a solution containing 0.12 mol/L of NH4Cl and 0.03 mol/L of NaOH (pKa of is 9.25)? My solutions manual says that: NH3=0.03 and NH4+=0.09, since we know that [NH4+] + [NH3] = 0.12 mol/L and that NaOH completely dissociates to give [OH-]= 0.03 mol/L.

1. At Equivalence  100 mL of 0.1000 M CH3COOH is titrated with 0.1000 M NaOH. Suppose that 30 mL of NaOH has been added. pKa = 4.75.  100 mL of NaOH has now been added to the acid.  How many moles of CH3COO- have been created?  moles. What is the pKb for the base?  What is the pH at this point in the titration? 2.

Calculate the pH of 500 ml of a 10 mM solution of sodium borate, pH 9.0 after the addition of 1.0 ml of a 1.5 M solution of NaOH. pKa of boric acid=9.24. What will the final pH be if you add 1.0 ml of 1.5 M HCl? Contrast the results for HCl and NaOH and explain the difference.

What is the pH of a solution containing 0.12 mol/L of NH4Cl and 0.03 mol/L NaOH (pKa of NH4+/ NH3 is 9.25)? I keep getting pH=8.6 when I know I am meant to be getting pH=8.77 however am unsure how to get there. Thanks

You are to devise an experiment to estimate its approximate pKa, without using a pH meter. Materials that are available for you to use are: a solution of NaOH with a precisely known concentration, a volumetric buret and other common lab glassware, a digital analytical balance, water, pH paper, and standard acid-base indicators.

Data Table 1: Determination of Equivalence Point Trial 1 Trial 2 4 mL 4 mL 112 117 Volume of Unknown Weak Acid (mL) Total Number of Drops Required to Reach Equivalence Point Average Number of Drops 113 Data Table 2: Titration Curve Values pH Value Trial 2 pH Value (Average) 4 4 Drops NaOH PH Value Trial 1 Added Half- 4 Equivalence Point ...

1. pH of a solution containing 0.12 M NH4Cl and 0.03 M NaOH (pKa of NH4+ = 9.25) 2. A biochemist makes up 100 mL of a 0.100 M solution of hisitidine at a pH of 5.40. She then adds 40 mL of 0.10 M HCl. What is the pH of the resulting solution? 3. Consider the ionizable groups of glutamic acid and draw all possible forms of this amino acid.

(pKa for acetic acid = 4.74; Ka for acetic acid = 1.8 x 10-5) Calculate the pH of a buffer solution prepared by mixing 30 mL of 5% acetic acid with 10 mL of 0.5 M NaOH. There are 3 steps to solve this one.