Could you show me how you solved to get pH of each solution: Solution A has [H3O+] = 7.2à?10-5 Solution B has [H3O+] = 7.2à?10-4 Solution C has [OH-] = 3.0à?10-11 Solution D has [OH-] = 6.5à?10-11 (i) Which solution has the highest pH? (ii) Which solution is the least acidic? (iii) Which solution is the most
One of the impacts of fossil fuels is an increase in acid deposition (or acid rain as many people refer to it). The following exercise asks you to calculate how much lime (an alkaline rock, not the tasty green fruit) it would take to increase the pH of a small lake. Consider a small lake in the Adirondack region of New York
Calculate the pH with the correct significant figures of: a. A solution prepared by dissolving 2.55g (NH4)2SO4 (FW=132.141;Ka of NH4 = 5.7x10^-10)in 100.0 ml of water, adding 100 ml of 0.201 M NaOH, and diluting to 500.0 ml with water. b. H2C, is a weak diprotic acid with a Ka1=1.2X10^-3 and Ka2 = 8.9x10^-9. A 30.00 ml
What is the minimum pH at which aluminum hydroxide, Al(OH)3 will precipitate from a 0.020 M Al(NO3)3 solution. Consider activity effects. The Ksp for Al(OH)3 is 3x10^(-34). Assume the pH can be changed without increasing the solution volume.
Sodium chloride is obtained when sodium carbonates react with hydrochloric acid. The equation for the reaction is: Na2CO3 = 2HCl --> 2NaCl + CO2 + H20 Calculate the mass of sodium chloride that can be obtained when 5 g of sodium carbonate is completely decomposed. (RAM = C=12, 0 = 16, Na = 23)
Sucrose decomposes in acid solution, according to the first order rate law, to give Glucose and fructose. If the half life for the reaction is 3.33 hours at 25 degree celcius, what fraction of a sample of sucrose would remain after 9 hours ?
1. Identify each of the following substances as strong electrolyte, weak electrolyte, or nonelectrolyte: Ba(NO_3)_2 Ne NH_3 NaOH. 2. Predict and explain which of the following systems are electrically conducting: solid NaCl molten NaCl an aqueous solution of NaCl. 3. Characterize the following compounds as solu
Please answer the three questions in the attachment. I'm having trouble with this acid-base chapter. Thanks!
Problem: A flow chart detailing some reactions of an Ester. Solution: Details the missing parts of the flow chart and provides answers to related questions.
Using the flow chart provided (see attachment Brainmass Problem 6). Please answer the following. 1) Give the structures and names of compounds 1-7. 2) Estimate the pH of compound 3? 3) Explain with an equation the reaction in which compound 4 is changed to 6 4) What are the key differences between the hydrolysis o
A solution has a pH of 6.72. Calculate the concentration of hydrogen ions in the solution.
Calculate the pH when 25.0 mL 0.20M HCl is titrated with 30.0mL of .20 M NH3 Kb(NH3)=1.8x10^-5.
Determining the type of acid and base (strong or weak) that decreases in pH at equivalence in a titration experiment.
In a titration experiment, if the initial solution pH is 9.0 and equivalence point occurs at pH 3.0, then the reaction corresponds to a. the titration of a strong acid by a strong base b. the titration of a strong base by a strong acid c. the titration of a weak acid by a strong base d. the titration of a weak ba
Which of the following solutions is not a buffer? a. 125mL of 0.200M HCl added to 200mL of 0.400M CH3CO2- b. 200mL of 0.400M HCl added to 125mL of 0.200M CH3CO2- c. 200mL of 0.500M NaOH added to 200mL of 1.000M HF d. 100mL of 0.500M H2PO4- added to 100mL of 0.100M HPO42- e. 100mL of 0.200M HF added to 300mL o
1.) A saturated solution of calcium sulfate can be prepared by diluting 0.29g of CaSC4 to 250mL. what is the Ksp of calcium sulfate? 2.) At pH 10.0, only 0.019g of MgCl2 will dissolve per 1L of solution. What is the Ksp of magnesium hydroxide, Mg(OH)2?
25.00mL of 0.50M NaOH is titrated with 0.50M HCl. What is the pH of the solution after 50.00mL of HCl 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?
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?
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)
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