3) Ammonia, NH3, is toxic to a wide range of aquatic organisms including snails, insects,and fish. The ammonium ion, NH4", is much less toxic since the cation does not diffuserapidly across cell membranes. The US EPA limit for total ammonia in natural waters is1.9 mg/L at pH 7.a. What is this limit in molar units?b. What is the concentration of NH3 at pH 7?c. What is the concentration of NH3 at pH 6?d. Why is the EPA limit for total ammonia dependent on the water pH?

The equation establishing the relationship between ammonia (NH3) and ammonium (NH4+) in water is as…

Answered: Ammonia, NH3, is toxic to a wide range…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Consider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate its pH. b. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. c. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.
A 1.00 g sample containing NaHCO3 was dissolved in water and titrated using 0.500 M HCI. The sample solution required 12.5 mL of the titrant solution to reach endpoint. Assuming that only NaHCO3 reacts with HCl, how much of NaHCO3 is present in the sample? g
What is the concentration in % (w/v) of a solution prepared from 50.0 g NaCl and 2.5 L of water? A. 5.0 % B. 2.0 % O C. 0.020 % D. 0.050 % E. 0.50 %
3. a) An aqueous solution is 3.50% by mass potassium bromide, KBr, and has a density of 1.02 g/mL. The molality of potassium bromide in the solution is _________m. b)An aqueous solution of magnesium nitrate has a concentration of 0.474 molal. The percent by mass of magnesium nitrate in the solution is _________%. c)An aqueous solution of cobalt(II) bromide has a concentration of 0.153 molal. The percent by mass of cobalt(II) bromide in the solution is _________%.
What is the concentration in % (w/w), of a solution prepared by mixing 50.0 g NaCl and 150.0 g water? A. 0.250 % B. 33.3 % C. 40.0 % D. 25.0 % E. 3.00 %
An aqueous solution contains 0.34 M potassium cyanide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.34 mol HCI04 0.16 mol NaOH 0.33 mol KCIO4 0.16 mol HCIO4 0.33 mol HCN
You just made a 1.5M permanganate solution. What concentration is your potassium permanganate solution in percent? "K: 39.10 g/mole" "Mn: 54.94 g/mole" "O: 16 g/mole" "MW of KMnO4 is 158.04 g/mole" O a. 0.24% Ob. 20.1% O c. 15.8% O d. 23.7% O e. 2%
I want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM MgCl2. I have the stock solutions 1 M glycene, 1 M MgCl2, 1 M ZnCl2, and 10 M NaOH. My final volume of buffer solution needs to be 250ml. how much (in ml) of each solution should i put into my buffer?
1. We have a 10% NaCl stock solution. Our nutrient solution is 3 mM for NaCl. How many ml of stock solution do we need for 500 ml of our solution nutrients? (MNaCl:58.49) 2. We work with a NaOH stock solution. We have to dilute 1: 4 to obtain a 2.5% solution. Find the concentration of the stock (% and mg/ml)
At 39.9ºC, a solution of ethanol (XetOH = 0.9006, P * etOH = 130.4 Torr) and isooctane (P * iso = 43.9 Torr) forms a vapor phase with YetOH = 0.6667. The total pressure is 185.9 a. Calculate the activity and the activity coefficient of each component.b. Calculate the total pressure the solution would have if it were ideal.c. Comparing the ideal pressure to the actual pressure, what does this indicate about the molecular interactions?
An analysis done on total Mn2+ of an industrial effluent is found to be 8.5 mmol L-1. The effluent will be discharged in a lake of 15 mg L-1 fulvic acid (FA) content. What is the fraction of FA expected to bind to Manganese at pH-5. Assume that Mn2+ is the only cation present in Water Lake and that its concentration is 1/10th of that of the effluent after being diluted in the lake. Binding sites of FA = 4.5 mmol g -1 and K'f (MnFA) at pH 5 = 5.0 x 10^3 Select one: A. 0.51 B.51% C. None of the suggested answers D. 0.62 E.81%
Based on the Henderson-Hasselbalch equation (shown below), calculate the pH when half of a solution of acetic acid is dissociated to acetate (the pKa of acetic acid is 4.76). A. 1.00 B. 3.76 C. 4.76 D. 5.76

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