The percent concentration of a solution is a ratio of the amounts of dissolved solute and solution, expressed as a percentage. The percent concentration of a solution can be written generally as % concentration = amount of solute amount of solution ×100% Depending on the situation, a percent concentration might be calculated for mass/mass, volume/volume, or mass/volume. Part A Calculate the mass percent of a solution that is prepared by adding 49.8 g of NaOH to 331 g of H2O. Express your answer numerically. View Available Hint(s) %(m/m) Part B Calculate the mass/volume percent of a NaCl solution in which 122 g of NaCl is dissolved in enough water to give a total volume of 2.26 L. Express your answer numerically. View Available Hint(s) %(m/v)
What is the concentration of B expressed in terms of A if the Kd is 37.0 uM, and the concentration of AB is 16.0 uM? A+B <=> AB B = 430/A B = 592/A B = 0.592/A B = 0.430/A B = 2.31/A
Which of the following are true regarding RTKs (there may be more than one correct answer, select all that apply). An active RTK is always phosphorylated An active RTK can phosphorylate other proteins An inactive RTK dissociates from the membrane An active RTK always has GTP bound directly to it
The concentration of particulate matter (in parts per million) t hours after a factory ceases operation for the day, is given by the following formula, C(t). Find the average concentration for the period from t = 0 to t = 6. C(t) = 18 ln(t+11) (t+11)2 The average concentration of particulate matter, for the time period from t = 0 to t = 6, is approximately parts per million. (Do not round until the final answer. Then round to four decimal places as needed.)
Consider the following elementary reaction: NO2(g) + O3(g) → NO3(g) + O2(g) Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of O2 in terms of k1, k−1, and the equilibrium concentrations of NO2, O3, and NO3. [O2] =
A drug's concentration in a patient's blood, in micrograms per milliliter, can be modeled by the function C(t) = 8t 0.01t2+5.3 where t is the time, in minutes, since the drug is injected. The drug's concentration will be milligrams per milliliter 25 minutes since the injection. Round your answers to two decimal places if needed. When the drug's concentration decreases to 9.23 milligrams per milliliter, it's time to give the patient another injection. The nurse should wait for minutes before another injection. Round your answers to an integer if needed. If no re-injection is applied, in the long term, the drug's concentration will be milligrams per milliliter.
A titration is a way to determine the concentration of an unknown base by using an acid with a very accurately known concentration. In a strong acid/strong base titration, the equivalence point is at pH7, and the moles of acid are equal to the moles of base. If 10.351 mL of 0.92547 M H2SO4 were used to bring an unknown concentration of 15 mL of CsOH to a pH of 7.01 , what was the concentration of the CsOH?
What is the final concentration of chloride ion, [Cl−], in a solution made by mixing 158 ml of 0.200 M NaCl with 200 mL of 0.150 M MgCl2? A) [Cl−] = 0.350 M B) [Cl−] = 0.187 M C) [Cl−] = 0.424 M D) [Cl−] = 0.192 M E) [Cl−] = 0.256 M
How many milliliters of a 0.400 M NaCl solution would you need to add to 1.00 L of a 2.0×10−2 M AgNO3 solution to completely precipitate all of the silver as AgCl(s) ? A) 180 mL B) 50.0 mL C) 240 mL D) 36.0 mL E) 120 mL Exam tip: How many grams of AgCl would precipitate by mixing 50 mL of 0.4 M NaCl with 80 mL of 0.2 M AgNO3? You'll need to determine the limiting reactant first. FWT of AgCl = 143.31 g/mol Answer: 2.3 g AgCl. This is not the actual exam question but is given for additional practice.
What is the concentration of NH2−CH2−COO−in a 2.9 M Glycine buffer, pH 11.60? (pKa's for Glycine acid are 2.35 and 9.78) Give your answer to 3 decimal places.
Consider the concentration cell shown below. Calculate the cell potential at 25∘C when the concentration of Ag+ in the compartment on the right is the following. a. 1.0 M b. 2.0 M c. 0.10 M d. 4.0×10−5 M e. Calculate the potential when both solutions are 0.10 M in Ag+. For each case, also identify the cathode, the anode, and the direction in which electrons flow.
A solution has a concentration of 66.6% (m/v) and volume of 225 mL; what is the mass of the solute in this solution? 29.6 g 15.0 g need more information 1.50×102 g 33.8 g