25.00mL of 0.200M HCl is titrated with 0.200M NaOH. What is the pH of the solution after 22.50 mL of NaOH has been added?
A buffer is prepared by adding 1.50x10(exponent 2)mL of 0.250M NaOH to 2.50x10(exponent 2)mL of 0.350M weak acid, HB. The solution is diluted to 1.00L. If the pH of the resulting solution is 5.55, what is the pKa of the weak acid?
The pH of 0.500M ammonium chloride, NH4Cl, is 4.78. What is the value Ka for this acid?
The pH of 0.350M benzoic acid, HC7H5O2 is 2.32. What is the pKa for this acid?
The pH of 0.400M sodium nitrate is 8.42. What is the kb for this base?
A 1.000-g sample of benzoic acid, C7H6O2, is burned in a bomb calorimeter. The temperature of the calorimeter increases by 7.53 degrees Celsius. What is the heat capacity of the calorimeter in units of kJ degrees Celsius -1? Please note that (3.09)(10^3)kJ of heat are liberated per mole of benzoic acid combusted.
What volume of .320 M HCL (hydrochloric acid) is required to react with 25 mL of .180 M Ba(OH)2 (barium hydroxide)?
What is the oxidation number of chlorine in perchloric acid, HClO4?
25.00ml of a 0.200M nitric acid solution is added to 50.00ml of a 0.100 M sodium hydroxide solution. What is the pH of the solution?
1.50g of sodium flouride is dissolved in water and the solution is made up to 250.00mL in a volumetric flask. What is the pH of the solution? (Ka for HF 1.0e-3) 1.0 x 10 to the power of-3.
What volume (in mL) of 0.37M HCI solution must be added to 265.00 mL 0.29M ammonia solution to give a buffer solution with pH 9.1? (Kb for ammonia 1.80e-5) 1.80 x10^-5
40.4mL of 0.100M nitric acid solution is added to a 1.00L volumetric flask and the solution is made up to the mark. What is the pH of the solution?
What is the new pH if a drop containing 0.001 moles of HCl is added to 100.00 ml of a solution 0.100M in each of acetic acid and sodium acetate? (ka for acetic acid 1.75e-5) 1.75x10^-5
What is the percent ionization of the acid in a 0.0008M solution of nitrous acid (HNO2) (ka 4.0e-4)? (4 times 10 to the power of -4)
50ml 0.200M acetic acid solution is added to 50.00ml .200M sodium hydroxide solution. What is the pH of the solution? (ka for acetic acid 1.75e-5) 1.75 times 10 to the power of negative 5
What is the pH of a 0.0001M solution of formic acid? (HCO2H) (ka= 1.77e -4) 1.77x10 to the power of negative 4)
How do I make household acid and base indicators? The process is included.
Can a neutral solution be at pH 8 ? Explain pH.
1) The lead batteries in cares are based on the following pair of half-reactions PbO2 (s) + HSO4- (aq) + 3H+ (aq) + 2e- --> PbSo4 (s) + 2H2o (l); E=1.63V PbSO4(s) + H+ (aq) + 2e- ---> Pb(s) + HSO4- (aq); E= -0.293V a) Write the balanced cell reaction that occurs when a lead battery generates current. b) Write the
Which is more acidic, a solution with a pH = 4.74 or a solution that has [H+] of 2.5x10-5M?
What is the difference between a strong acid and a weak acid? Give one example of each. What is meant by the ionic product for water, Kw? Define pH and hence calculate the pH of a solution of a) 0.01 M hydrochloric acid b) 0.1 M sodium hydroxide c) 0.2 M sulphuric acid d) 0.1 M butanoic acid, given that Ka = 1.51 x 10-5
Understanding the Concepts of pH and pOH, and the Relationships Surrounding Concentration, Moles, Molarity, and Number of Molecules
An aqueous solution of an unknown substance has a pH of 3.0. If you have 0.25 L of the substance, how many (a) H+ ions, and (b) OH-ions, are present?
Determine the pH of an aqueous solution prepared by mixing 50 mL of .125 M KOH with 50 mL of .125 M HCl while maintaining the temperature of the the system at 50 degrees C.
The pKa of HCN is 9.2. Calculate the Ka of HCN.
Amide ion (H<sub>2</sub>N-) is a stronger base than the hydroxide ion (OH-). Which would you expect to be a stronger acid, NH<sub>3</sub> or H<sub>2</sub>O? Why?
Picric acid (C<sub>6</sub>H<sub>3</sub>N<sub>3</sub>O<sub>7</sub>) has a pKa of 0.3. Formic acid (CHO<sub>2</sub>H) has a pKa of 3.7. Which is the stronger acid?
Ascorbic acid (vitamin C) has a pKa of 4.2 at 24 degrees Celsius. State the pH of the solution when the ratio of unprotonated to protonated forms of ascorbic acid is (a) 1:1 (b) 1:10 (c) 10:1 (d) 1:3 (e) Which form of ascorbic acid predominates at physiological pH?
Determining the pH of an acid and base in various situations by working with concentrations. A multi-step question.
Part 1: What is the pH of a solution of 1M HCO3 and 1M CO3? Part 2: What is the pH if it was mixed with an equal volume of water? Part 3: What is the pH if it was mixed with an equal volume of 0.001 M HCl? Part 4: What is the pH if it was mixed with an equal volume of 0.001 M NaOH?