Interpretation:
The
Concept Introduction:
Titration: It is a quantitative analysis method used to express the concentration of acid or base present in the solution.
For an
That is,
Normality: It generally expresses the concentration of acid or base as equivalents of acid or base present in one liter of the solution.
Equivalent of Acid: Generally, 1 equivalent of ion is the number of ions which has charge of one mole.
It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.
Want to see the full answer?
Check out a sample textbook solutionChapter 10 Solutions
Fundamentals of General, Organic, and Biological Chemistry (8th Edition)
- The pH of black coffee is 5, and that of milk of magnesia is 10. Is the coffee twice as acidic as milk of magnesia?arrow_forwardYou need to prepare an acetate buffer of pH 5.43 from a 0.621 M acetic acid solution and a 2.95 M KOH solution. If you have 730 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.43? The pKa of acetic acid is 4.76. Be sure to use appropriate significant figures.arrow_forwardWhat mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.arrow_forward
- What would be the working stock concentration (in molarity) if you diluted 250 uL of a stock concentration of 10 uM in a total volume of 1 mL?arrow_forwardA 25.00 mL sample of 0.320 M LIOH is titrated with 0.750 M HNO3 at 25 °C. Calculate the initial pH before any titrant is added. pH = Calculate the pH of the solution after 5.00 mL of the titrant is added. pH =arrow_forwardCalculate the molarity of dilute Ca(OH)2 solution if the titration of 30.00 mL of 0.05231 M HCl required 24.76 mL of the acid. An 0.2500 g hydroxide tablet sample submitted in the lab used 36.75 mL during titration. How much is the hydroxide in mg present?arrow_forward
- If 4 mL of 1 M NaOH is added to 100 mL buffer, would it still be a usable buffer according to the conventions? Explain why or why not.arrow_forwardAn aqueous solution of 0.2100 g of a mixture containing potassium cyanide and potassium chloride required 14.56 mL of 0.1000 M silver nitrate to produce a faint permanent turbidity; 30.00 mL more of the silver nitrate was added (an excess) and the precipitate of AgCl and AgCN filtered off from the solution. The filtrate and washings were titrated with 13.06 mL 0.1000 M thiocyanate solution. Calculate the percentages of KCl and KCN in the sample. Note: the appearance of faint turbidity indicates the formation of Ag(CN)2-arrow_forwardHow much water must be added to 300 mL of an aqueous solution of 0.2 M acetic acid in order to double the degree of ionization? Take the acid ionization constant of acetic acid to be 1.8 x 10-5.arrow_forward
- Draw titration curve for compound X when NaOH equivalence(s) is/are added. Indicate the buffering region(s) with a box.arrow_forwardA 35 mL of solution of hydrochloric acid is neutralized by 15 mL of 0.5 M potassium hydroxide. What is the concentration of hydrochloric acid? The balanced equation is HCI + KOH - H,O + KCI O 0.75 M O 0.25 M O 0.214 M O 0.786 Marrow_forwardWhat is the pH of a 0.25 M solution of acetic acid, Ka = 1.8 x 105. What percentage of the acid is dissociated?arrow_forward
- Human Biology (MindTap Course List)BiologyISBN:9781305112100Author:Cecie Starr, Beverly McMillanPublisher:Cengage Learning