8.34 and [HCO3-] = 183Suppose a particular water sample is known to have pHmg/L.(a) Estimate or calculate the molar concentrations of HCO3¬, H+, OH-, H,CO3, andCO32-. Hint: yes, you have enough information to do these calculations.(b) Suppose that the only other ion present in the water is sodium, Na+. Estimate orcalculate the molar concentration of Na+ that would be required to ensure chargeneutrality in the water: [Na+] + [H+] = [OH-] + [HCO3-] + 2[CO32-].(c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity asnormality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinityin the text book if we don't get to it in class.(d) Repeat parts (a)-(c) if the pH is 8.34 (as it was before), but now the concentrationof bicarbonate is [HCO3-] = 30 mg/L.(e) Now suppose you have two beakers. In the first beaker, you put 99 mL of the firstwater sample (183 mg/L bicarbonate) and you add 1 mL of hydrochloric acid (HCI).The concentration of the HCl (before addition to the water sample) is 0.1 M, whichis also equal to 0.1 N. In the second beaker, you put 99 mL of the second watersample (30 mg/L bicarbonate) and you add 1 mL of HCl. You allow both mixturesto equilibrate, and then you measure the pH in both beakers. What doyou thinkyou will see? Why? Hint: it is possible to actually calculate the pH in each beaker,but that is a pretty complicated calculation, and it is beyond the scope of ENV 4001;try for a qualitative answer here. Will the pH go up or down in the first beaker? Bya little or by a lot? Why? What about in the second beaker? Why?

Answered: Image /qna-images/answer/f8015601-33cc-4db0-ab6b-76cd52daf07f.jpg

Suppose a particular water sample is known to have pH = 8.34 and [HCO3-] = 183 mg/L. (a) Estimate or calculate the molar concentrations of HCO3-, H+, OH-, H2CO3, and CO3²-. Hint: yes, you have enough information to do these calculations. (b) Suppose that the only other ion present in the water is sodium, Na+. Estimate or calculate the molar concentration of Na+ that would be required to ensure charge neutrality in the water: [Na+] + [H+] = [OH-] + [HC03-] + 2[CO3²-]. (c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity as normality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinity in the text book if we don't get to it in class. (d) Repeat parts (a)–(c) if the pH is 8.34 (as it was before), but now the concentration

Suppose a particular water sample is known to have pH = 8.34 and [HCO3-] = 183 mg/L. (a) Estimate or calculate the molar concentrations of HCO3-, H+, OH-, H2CO3, and CO3²-. Hint: yes, you have enough information to do these calculations. (b) Suppose that the only other ion present in the water is sodium, Na+. Estimate or calculate the molar concentration of Na+ that would be required to ensure charge neutrality in the water: [Na+] + [H+] = [OH-] + [HC03-] + 2[CO3²-]. (c) Estimate or calculate the alkalinity of the water sample. Report the alkalinity as normality (eq/L) and as mg/L of CaCO3. You can look up an equation for alkalinity in the text book if we don't get to it in class. (d) Repeat parts (a)–(c) if the pH is 8.34 (as it was before), but now the concentration

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 58P

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Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following statements best describes what happens? a. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat. b. The H+ from the HCl reacts somewhat with the A from the NaA to make HA, while the HA is dissociating. Eventually you have equal amounts of everything. c. The H+ from the HCl reacts somewhat with the A from the NaA to make HA while the HA is dissociating. Eventually all the reactions have equal rates. d. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat until too much H+ and A are formed, so the H+ and A react to form HA, and so on. Eventually equilibrium is reached. Justify your choice, and for choices you did not pick, explain what is wrong with them.
Acetominophen, HC8H8NO2 (MM=151.17 g/mol), is the active ingredient in Tylenol, a common pain reliever. A solution is made by dissolving 6.54g of acetaminophen in enough water to make 250.0 mL of solution. The resulting solution has a pH of 5.24. What is the Ka for acetaminophen?
(a) Acid rain is no threat to lakes in areas where the rock is limestone (calcium carbonate), which can neutralize the acid. Wherethe rock is granite, however, no neutralization occurs. How does limestone neutralize acid? (b) Acidic water can be treated withbasic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass oflime, CaO, needed to adjust the pH of a small lake (V = 4 x 109 L) from 5.0 to 6.5. Why might more lime be needed?
1. If you mixed 375 ml of 5.2 M HCO2H with 375 ml of 5.2 M CH3CO2-, what would be the final pH? 2. What is the pH of a 3.65 L solution of 4.55 M NH3? How many grams of LiOH would it take in the same amount of volume to get the same pH?
13.2) Acetaminophen, HC8H8NO2 (MM = 151.17 g/mol), is the active ingredient in Tylenol®, a common pain reliever. A solution is made by dissolving 8.68 g of acetaminophen in enough water to make 410.0 mL of solution. The resulting solution has a pH of 5.29. What is Ka for acetaminophen?
Sodium hypochlorite solution, sold as “chlorine bleach,” ispotentially dangerous because of the basicity of ClO⁻, the active bleaching ingredient. What is [OH⁻] in an aqueous solution that is 6.5% NaClO by mass? What is the pH of the solution? (As-sume d of solution= 1.0 g/mL.)
The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of H2CO3/HCO3− is required to obtain a pH of 7.40, the pH of blood? (Assume that the Ka of H2CO3 is 4.4 ✕ 10−8.)
Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution containing 7.50 g of this salt is diluted with water until it reaches a pH of 8.18.What is its final volume? Give one example of a salt whose solution is expected to be acidic and briefly explain why. Give one example of a salt whose solution is expected to be basic and briefly explain why. You cannot reuse the compound in a) and b) to answer c) and d).
The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid?
The hypochlorite ion, ClO-, acts as a weak base. (a) Is ClOa stronger or weaker base than hydroxylamine? (b) When ClO- acts as a base, which atom, Cl or O, acts as the proton acceptor? (c) Can you use formal charges to rationalize your answer to part (b)?
How many moles of NH4Cl would need to be added to 441.6 mL of 1.43 M NH3 to produce a solution with a pH equal to 8.66?
The methoxide ion, CH₃O⁻, and amide ion, NH₂⁻, arevery strong bases that are “leveled” by water. What does thismean? Write the reactions that occur in the leveling process.What species do the two leveled solutions have in common?