Phosphate buffer solution, which is used in preparing the BOD dilution water is prepared by dissolving 0.85 g of monobasic potassium phosphate (KH2PO4), 2.175 g of dipotassium hydrogen phosphate (K2HPO4), 3.34 g of disodium hydrogen phosphate heptahydrate (Na2HPO4.7H2O), and 0.17 g of ammonium chloride (NH4CI) in about 50 mL distilled water before further diluting to 100 mL using distilled water. Assuming that all phosphate compounds are 100 % (w.w) pure and dissociated completely in the form of free phosphate ions (PO43-) in water, calculate the concentration in ppm of the total free phosphate ions (PO43-) in the 100 mL solution. Given that the atomic weight for Nitrogen, N is 14.0067 g/mole; Hydrogen, H is 1.0079 g/mole;, Cl is 35.453 g/mole; Phosphorus, P is 30.9738 g/mole; Oxygen, O is 15.9994 g/mole; Sodium, Na is 22.9897 g/mole; Potassium, K is 39.0983 g/mole

Phosphate buffer solution, which is used in preparing the BOD dilution water is prepared by dissolving 0.85 g of monobasic potassium phosphate (KH2PO4), 2.175 g of dipotassium hydrogen phosphate (K2HPO4), 3.34 g of disodium hydrogen phosphate heptahydrate (Na2HPO4.7H2O), and 0.17 g of ammonium chloride (NH4CI) in about 50 mL distilled water before further diluting to 100 mL using distilled water. Assuming that all phosphate compounds are 100 % (w.w) pure and dissociated completely in the form of free phosphate ions (PO43-) in water, calculate the concentration in ppm of the total free phosphate ions (PO43-) in the 100 mL solution. Given that the atomic weight for Nitrogen, N is 14.0067 g/mole; Hydrogen, H is 1.0079 g/mole;, Cl is 35.453 g/mole; Phosphorus, P is 30.9738 g/mole; Oxygen, O is 15.9994 g/mole; Sodium, Na is 22.9897 g/mole; Potassium, K is 39.0983 g/mole

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The concentration of SO42– ions in a 45.0 mL sample of seawater is determined by adding a solution of BaCl2 and precipitating the SO42– as BaSO4. After the precipitate is filtered from the solution, it is dried and weighed. If the mass of BaSO4 recovered is 0.315 g, what is the sulfate concentration of the seawater sample? Express your answer in mmol/L.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 43. mg of oxalic acid (H₂C₂O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 10.1 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. OM x10 X Ś ? olo Ar
A chemistry student weighs out 0.361 g of ascorbic acid (H₂C,H,O), a diprotic acid, into a 250. ml. volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1700 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. ? X do
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 214.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 91.8mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
When 1.50 L of 0.225 M NaOH is mixed with 2.00 L of 0.450 M FeCl3 and the following reaction occurs: 3NaOH(aq)+FeCl3(aq)→3NaCl(aq)+Fe(OH)3(s) What is the theoretical mass of the precipitate that will be produced?
You prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC,H,O,, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC̟H,O, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 19.14 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?
Determining the volume of base needed to titrate a given mass of acid A chemistry student weighs out 0.193 g of lactic acid (HC3H₂O3) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1400M NaOH solution. 1/5 mL Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits. X Allison
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 233. mg of oxalic acid (H₂C₂O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 63.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed. OH(aq) + OH¯(aq) → H₂O(l) O H+ (aq) + OH(aq) + 2 K+ (aq) + SO4²-(aq) → H+ (aq) + OH¯(aq) + K₂SO4(s) O No reaction occurs. O 2 K+ (aq) + SO4²- (aq) → K₂SO4(s) H+ (aq) + OH Taq) + 2 K+ (aq) + SO42 (aq) → H₂O(l) + 2K+ (aq) + SO4²- (aq)
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 276. mg of oxalic acid (H₂C₂O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 138.7 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits. M X 3
Which of the following is a complete balanced equation for the reaction between a nonmetal oxide and water? ○ SO3 (g) + H2O (l) → H₂SO4 (aq) Ca (s) + 2 HBr (aq)· → CaBr2 (aq) + H2 (g) MgO (s) + H2O (l) → Mg(OH)2 (aq) ○ P4010 (g) + H2O (l) → H3PO4 (aq)
the number of moles of Aluminum in 1.3741 g was calculated to be 0.051 moles and that the chemistry student weighed out. For every mole of Aluminum that you start with, you can create one mole of Alum [KAl(SO4)2 ⋅12 H2O(s)]. What is the theoretical yield before drying the Alum precipitate?