Which of the following is a property of acid solutions? a. sour taste c. change red litmus to blue b. slippery feel d. more than one response is correct A 25.00 mL sample of hydrochloric acid solution, HCl, is titrated with 0.0512 M NaOH solution. The volume of NaOH solution required is 21.68 mL. What is the molarity of
The molar concentration of H+ ions in a solution is 5.8 × 10-9. The pH of the solution is a. 9.00 c. between 8.00 and 9.00 b. 5.80 d. between 9.00 and 10.00 A solution for which [OH-] = 3.0 × 10-10 is classified as a. acidic c. neutral b. basic d. more than one response is correct 10. A solution has a pH of 11.60. Th
A water solution is found to have a molar OH- concentration of 3.2 × 10-5. The solution would be classified as a. acidic b. basic c. neutral d. can't be classified What salt would be produced by the reaction of H2SO4 with LiHCO3? a. Li2S b. LiSO4 c. Li2SO4 d. Li2CO3 7. The molar concentration of OH in a water solution i
1) The Equilibrium constant Kp for the reaction 2SO2(g) + O2(g) --- 2SO3(g) Is 5.60 x 10^4 at 350 degrees C. The initial pressures of SO2 is 0.350 atm and the initial pressure of O2 is 0.762 atm at 350 degrees C. When a mixture equillibtrates, is the total pressure less than or greater than the sum of the in
1.) Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 x10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8? green red blue yellow violet 2.)The Ksp value for lead(II) chloride is 2.4 x 10-4. What is the mol
1. If the pH of an aqueous solution is 8.23, what are the hydrogen- and hydroxide-ion concentrations of this solution? 2. If 7.40 grams of Ca(OH)2 is dissolved in sufficient water to make 100mL of solution, what is the hydroxide-ion concentration of this solution? 3. What is the hydroxide-ion concentration, the pH, and the hyd
Calculate the volume (100mL) of the 0.1M dihydrogen phosphate (monobasic)and the volume of the 0.1M monohydrogen phosphate (dibasic) that are required to make a buffer at pH 7.4. Ka Monobasic=6.2x10^-8 Ka dibasic=4.8x10^-13
1.)If I wanted to make 50ml of a 1/20 dilution of a 0.1 M salt solution, how would I go about doing this; meaning what volume of 0.1 M salt solution and what volume of water would I need to add? 2.) If I wanted 10ml of a 1mM nitrophenol solution and all I had on hand is a 50 mM nitrophenol solution, how would I make it? 3.
A 10.0ml sample of 0.010M H2SO4 is titrated with 0.020M NaOH. What is the pH of the solution after 30.0mL of base have been added?
I'm given the Ka and concentration to calculate the pH then find % ionization. I utilized an ice table and made the assumption that x << the # i'm working with, however, when I check the assumption... its not < 5% snd plugged my #'s into the quadratic formula and both #'s check... when one # is usually eliminated and I'm left wi
1. balance equations:----> (equals heat ) NaNO3 ----> NaNO2 + O2 SiO2 -----> no reaction PbO2 -----> PbO + O2 MgO -------> no reaction KClO3 -----> KCl + O2 2 .Rocks and soil on the Moon, as on the Earth, consist mainly of silicon-oxygen compounds, called silicates. What is the chance that astronauts could easil
Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known? Explain. Answer needs to be in a 200-300 word response in essay form.
Calculate the number of O atoms in 1.50 g of glucose C6H12O6 a sugar. It is estimated that the day Mt. St. Helens erupted (May 18, 1980), about 4.0E5 tons of SO2 were released into the atmosphere. If all the SO2 were eventually converted to sulfuric acid, how many tons of H2SO4 were produced?
Procedure 1 Synthesis: 1. Take a crucible from the Glassware shelf and place it on the workbench. 2. Take a balance from the Tools shelf and drop it on the empty crucible. Record its mass. 3. Add 2g of Mg to the crucible and record its mass. 4. Remove the crucible from the balance. 5. Take a Bunsen burner from t
Consider the reaction below at 25 C: 3SO4^2- (aq) + 12H^+ (aq) + 2Cr (s) --> 3SO2 (aq) + 2Cr^3+ (aq) + 6H2O (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00
1.Consider the following cell at equilibrium: Mg(s) / Mg+2 (0.01 M) // OH- (?) / Mg(OH)2 (s) / Mg (s) Given: Mg+2 + 2e- ---> Mg(s) Eo = -2.360 V Mg(OH)2 (s) + 2e- ---> Mg(s) + 2 OH- Eo = -2.690 V a) Write each half-reaction and the net cell reaction. Find the standard net cell potential. b) Find the pH of the right cel
I need to determine the amount of HCl that would be necessary to reduce the pH of a wastewater from pH 5.0 to pH 4.0. The wastewater flow is given as 6,056,000 liters/day. The HCl is a 40% solution. The specific gravity of the HCl is given as 1.20. How do I determine both the mass and volume per unit time of HCl needed
QUESTIONS 1. Explain why it is not necessary to know the exact concentration of bromothymol blue in the solution. 2. The pKa value can also be determined from Figure 4 - explain. 3. The acid dissociation constant for bromothymol blue is dependent on ionic strength of solution. Determine the ionic strength of bromothy
The best way to ensure complete precipitation of tin(II) sulfide from a saturated solution of hydrogen sulfide is to... the answer is add a strong base. but I'm not clear on why this the right answer, can anyone explain?
A 2.0 x 10^-3 solution of manganese (II) sulfate is gradually made more basic by the addition of 1.0 sodium hydroxide solution. At what pH will manganese (II) hydroxide begin to precipitate? (Ksp= 2 x 10^-13) What is the balanced equation and how do you set the problem up?
Question 1: Using the Lewis concept of acids and bases, identify the Lewis acid and base in each of the following reactions: 1. Al(NO3)3 a) Lewis Acid b) Lewis Base c) Neither 2. H2O a) Lewis Acid b) Lewis Base c) Neither 3. CH3NH2 a) Lewis Acid b) Lewis Base c) Neither 4. HBr a) Lewis Acid b) Lew
PH Indicator Procedure #1 pH Indicators for Acids: 1. Take seven clean test tubes from the Glassware shelf and place them on the workbench. 2. Add 5 mL of 0.1M HCl and 5 mL of water from the Chemicals shelf to the first test tube. 3. Add 9 mL of water to the 6 remaining test tubes. 4. Pour 1 mL of the solution fr
Could someone please explain why in wastewater treatment that the oxidation of nutrients such as NH3 to NO ---> NO2 ----> NO3 occurs more completely at pH above 7.0 as opposed to pH below 7.0? In practice, the oxidation of ammonia (NH3) to nitrate (NO3) --- which is what we want --- definitely seems to occur better and faster
Please see the attached file for the fully formatted problems. KH = 3.3 x 10-7 Ka1 = 4.5 x 10-7 (carbonic acid) Ka2 = 4.7 x 10-11 (bicarbonate) Ksp = 5 x 10-9 (calcite) Assuming equilibrium between the atmosphere, seawater, and calcite: [H+]3 = KH2Ka12Ka2PCO22 2Ksp [HCO3-] = 2Ksp{H+]2
Based on the steps occurring in an acid-base reaction, which definition of acids and bases is most practical? Give three reasons for your choice.
Problem: Using the equivalent millimoles HCl/mg sample, the stoichiometry of reaction of HCl with NaOH (which I know is 1:1), and the molar mass of the hydroxide ion, report the gram equivalent OH- per gram of ...there is moreshow problem Using the equivalent millimoles HCl/mg sample, the stoichiometry of reaction of HCl with
Please provide solution for (a) and (b) with explanation of how it was derived. Early groups used Pb plumbing in their homes more than 2000 years ago. This Pb pipe has since corroded in the soil to form cerrusite (PbCO3) and hydrocerrusite ( Pb3(CO3)2(OH)2 ). Essington et al., 2004. The soil mineralogy of lead at Ho
Use the pE / pH diagram shown below to answer the following questions. What is the predominant form of cobalt at a pE of 7.0 and a pH of 4.0? at a pE of 7.0 and a pH of 10.0? at a pE of 2.0 and a pH of 9.0? at a pE of -3.5 and a pH of 5.5? List the forms of cobalt that would be transported in water? See the attached
A step by step method to prepare a buffer with a specific pH and concentration is given. This includes guidelines to find the conjugate acid/base pair, calculation of the buffer ratio using the Henderson-Hasselbalch equation, and the determination of mass of chemicals reagents required to prepare the buffer.
Sulfuric acid H2SO4(aq) is described as a strong acid whereas hydrofluoric acid HF(aq) is described as a weak acid. (a) (i) Describe what is meant by the terms strong and weak acid. (Two or three short sentences) (ii) Write fully balanced equations for the equilibrium dissociation of both sulfuric and hydrofluoric acids in