Suppose you had titrated with barium hydroxide instead of sodium hydroxide: Consider a 0.586 M aqueous solution of barium hydroxide (aq) for the next 4 problems. How many grams of Ba(OH)2Ba(OH)2 are dissolved in 0.191 dL of this solution? How many individual hydroxide ions are found in 13.4 mL of the original solution? What volume (in L) of the original solution contains 0.466 ounces of barium hydroxide dissolved in it? If 16.0 mL of water are added to 31.5 mL of the original solution, what is the new solution's molarity

9. You have 0.8557 g of an unknown monoprotic acid, HA, which reacts with NaOH according to the balanced equation HA + NaOH →→ NaA + H₂O If 43.48 mL of 0.1028 M NaOH is required to titrate the acid to the equivalence point, what is the molar mass of the acid?

6. A 0.4622-g sample of potassium hyd rogen phthalate was dissolved in 50 mL of deionized water and titrated to a phenolphthalein end-point with 19.48 mL of NaOH solution. What is the molarity of the NaOH? 7. Assuming that the density of vinegar is 1.012 g/m L, calculate the weight percent of acetic acid in vinegar if 23.85 mL of 0.1311 M NaOH was required to titrate 5.00 mL of vinegar. did HA nd dis 192 riw o asuuc no'noleauoetb s obulbo. As 900 900 4Coz2 anigll .asbtucf namheqx dini 209 (0 HoO Cag) (es) ibis 9C D DV 9 ballet tnabole A 9 u u 1oied qütenud orlf hi asiddud e 9t borsoog szib alddud sis ord nolt dsvawnlcrndtuodA 9l il blucwnolduloe HOe wans uoy nistqx3 Sipid oo! tstse : wot oo dhelom t bbs rg beau yilednobbos nsbile s est itbin ow osta isrl bsbne evicmi Srtulce HOs orts to yahelom orld ininetsb as 9 adant anoto toi n odslo 613 Exbiont Aorf

solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.

3. A 20.00 mL solution of a weak acid (0.05 M) weak acid was titrated with an aqueous solution of 0.01M strong base (sodium hydroxide). A) Calculate how much (in mL) of the 0.01 M NaOH will be required to neutralize the weak acid (20.00 mL 0.05 M) considering the weak acid is acetic acid. Show all steps, starting from the balanced chemical reaction. I HI 12 pH vs volume of titrant added 11 111 Volume of NaOH added o IV

1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume =   mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.  g/mol?

In the scary chemical storage room, you spot a bottle of potassium hydroxide solution, KOH, without a label noting its concentration! How terrible! (the nerve of some people...) Since you love chemistry, you decide to figure out its concentration by doing a titration. You add 5.00mL of 0.100M phosphoric acid to a flask and add KOH solution until it's all neutralized! If 5.00mL of potassium hydroxide solution were used in the titration, what is its concentration? 3.00 M     0.900 M     5.00 M     0.100 M     0.300 M

Oo.125. Subject:- Chemistry

12. In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 L if acid in a flask. You quickly add 20.00 mL of 0.0502 M NaOH but overshoot the endpoint, turning the solution a deep pink color. Instead of starting over you add an additional 30.00 mL of the acid, turning the solution colorless. It then takes 3.22 mL of the NaOH to reach the endpoint. a. Write the Molecular, Total Ionic, and Net Ionic Equations for this reaction. b. What is the concentration of the HNO3 solution? c. How many moles of NaOH were in excess after the first addition?