In our soda ash titrations, we used sodium carbonate and titrated it with HCl.  Solve the following problem with sodium bicarbonate.  A weight of 1.3250 g of sodium bicarbonate  is dissolved in 100.00 mL water.  If a 10.00 mL aliquot of the sodium bicarbonate solution is placed into an E-flask and titrated with 0.1034 M HCl, what should be the volume of HCl in ml to reach the endpoint?

The table has data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCl(aq), using a 0.299 mol/L sodium hydroxide standard solution.   Titration of 10.0 mL HCl(aq) with 0.299 mol/L NaOH(aq) Trial #1 #2 #3 #4 final burette reading (mL) 17.9 35.0 22.9 40.1 initial burette reading (mL) 0.3 17.9 5.9 22.9 volume of NaOH(aq) added (mL)         colour at endpoint blue green green green a)  Select the most consistent trials and calculate the average volume of titrantadded.b)  Calculate the concentration of the hydrochloric acid solution.

15.00 mL of 0.214 M oxalic acid, H2C2O4 ,solution was placed in an Erlenmeyer flask.  0.237 M KOH  solution was used to titrate the solution in the flask.   H2C2O4 is a diprotic acid and the Hs that are shown in blue are the Hs that will react with the hydroxide ion of a base. During the titration, KOH solution was added until ________ moles of H2C2O4 were in the reaction flask.

Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI

For your titration, it took 17.91 mL of unknown NaOH to react with 0.223 g of KHP. What is the molarity of the NaOH?

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution?   2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution?   3. What is the concentration of Ag+ in solution?

The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl.  How would you classify the species being titrated in this titration? diprotic weak base monoprotic weak base triprotic weak acid triprotic weak base diprotic weak acid monoprotic weak acid

7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation.           H3C6H5O7  (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?

24.16 mL of 0.2704 M sodium hydroxide is titrated with 29.00 mL of phosphoric acid.  Calculate the molarity of phosphoric acid.

Suppose that 42.00 mL of 0.150 M NaOH is added to 0.360 g of a weak acid, H3A.  The excess NaOH is then titrated with 23.40 mL of 0.120 M HCl.   What is the molar mass of the acid? a) 103 g/mol b) 241 g/mol c) 190 g/mol d) 310 g/mol