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- A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?(a) A 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH is titrated into the solution until the pH is exactly 5.0. What is the concentration of the titrant (NaOH)? (b) In the second step, enough 5.85 M nitric acid is added to the solution after the titration in part (a) is complete until the pH is one unit lower than the pKa of acetylsalicylic acid. What volume (mL) of nitric acid was added?When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s) 2NH4* + SO42- NH4* + NH3(aq) + H* SO2- + H2O → HSO4 + OH Ksp = 276 Ka = 5.70 x10-10 Кь 3 9.80 х 10-13 (a) (b) (c) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.
- The average blood pH is 7.40. The blood volume in humans, on average, is 5 liters. On average bicarbonate concentration in blood is 25 mM. A vinegar jar has a label that says its acetic acid concentration is 3.0%, meaning 3.0 g of acetic acid in 100 mL vinegar. (1) How many mL of vinegar does a person have to intake in order to lower the blood pH to 7.25? (2) if ALL the bicarbonate in 5.0 L of blood is neutralized by vinegar, how many mL of vinegar will be needed? (3) When all the bicarbonate ions are neutralized to carbonic acid, what will be the resulting blood pH? Note: pKa values for carbonic acid (diprotic acid) are 6.4 and 10.3, respectively.4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂The titration of 0.314 g of potassium hydrogen phthalate (KHP) requires 13.16 mL of a NaOH solution. What is the molarity of the NaOH solution?
- 6. A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 M acetic acid (CH3COOH) solution. (A) write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (B) Write the complete ionic equation for the reaction that occurs when few drops of sodium hydroxide solution are added to the buffer. Group of answer choices a.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq) (B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l) b.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq) (B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq) c.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq) (B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l) d.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq) (B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)A buffer solution was made by mixing 2.00 L of 1.500 M potassium nitrite with 1.00 L of 1.476 M nitrous acid. Ka (nitrous acid) = 4.5 x 10-4 For all to the following questions, write your answer as a normal number to three significant figures. (a) The molarity of the conjugate base in the solution at the instant of mixing is (b) The molarity of the weak acid in the solution at the instant of mixing is (c) The pH of the buffer after the mixing of the two solutions is Use the rules applicable to significant figures. (d) 19.04 g NaOH (39.9971 g/mol) is dissolved in this buffer solution (assume this causes no change in the volume of the solution) and reacts. The mole of added base remaining after the reaction is (e) At the same time, the moles of weak acid remaining is (f) At the same time, the moles of the conjugate base remaining is (9) THe pH of the buffer solution after the added base has reacted, is Use the rules applicable to significant figures.Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. H₂S (aq) + KOH(aq) → 2- 3C₂² 1 2 + (s) S 3 K Reset 4 (1) 5 6 LO O 7 (g) ㅈ H 8 9 11 (aq) Submit X 0 • x H₂O
- Suppose a 0.018M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium molarity of HPO4. You'll find information on the properties of phosphoric acid in the ALEKS Data resource. Round your answer to 2 significant digits. OMThe pHpH scale for acidity is defined by pH=−log[H+]pH=-log[H+] where [H+][H+] is the concentration of hydrogen ions measured in moles per liter (mol/L). (A) If there are 0.0079432823472428 mol/L of hydrogen ions in a certain substance, what is the pH of this substance?pH=pH= Round your answer to at least two decimal places. (B) If there are 0.003019951720402 mol/L of hydrogen ions in a different substance, what is the pH of this substance?pH=pH= Round your answer to at least two decimal places.For a 50.00 mL sample of a citrus beverage to reach the phenolphthalein endpoint, 17.62 mL of 0.04166 M NaOH is required. Determine the acidity of the sample in terms of grams of citric acid per 100 mL.