Qualitative Analysis Scheme NOTES SAVE YOUR DECANT! * YouR UNKNOWN WILL HAVE 1-4 TONS. * write down your observations here for the unknown Solution-be as detailed as Possible so you can use these notes to write your ion summary * write your Observations in a way that makes sense to you lie. A decant could be a cear I colorless solution), if you åre running out Of Space write additional observDirions in your lab notebook. * DO NOT LOSE THIS PAPER You WILL NEED TO INCLUDE IT IN YoUR LAB REPORT Hewe Pbt? Ag*, Hg,", Pb“, Ca*“, Mg**, Ba", NHa" NH3 19) SPecial +est (NHu) lit. Ped> bhe OBSERVATIONS (Wa) 12H PpY Decant Sand FOR Have NHY UNKNOWN UNK # SOLUTION NO Ppt (an,Mg 88 (2) Add (NH4)z SO4 Sdlid Decant Camplete Ba Soyis) white ppt Ppt. Ag, Hg?, Cat2, Mgr2,NHt PH must be basic gouhave Bazt PHZ8 (€) b) Add Said Deant ) Mg test b) you have Ca c) PH mvst be 7 ]! PH must M9LOH)z Cs) bluelpur ple Ppt be basic SAVE YOUR DECANT Have Mg2t

An analytical chemist weighs out 0.318 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 82.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol x10 x 3

What volume of 0.828 M HCl, in milliliters, is required to titrate 2.10 g of NaOH to the equivalence point?

By titration it is found that 114.3mL of 0.562M NaOH is needed to titration 48.0mL of Hcl. what is the concentration of the HCl in molarity?

Table 1: Titration Data Volume of magnesium hydroxide solution in Erlenmeyer flask Concentration of magnesium hydroxide 0.135 mol/L solution in Erlenmeyer flask Initial volume of nitric acid solution in burette Final volume of nitric acid solution in burette 10.Use the data in Table 1 to answer the folowing (a) Write the balanced chemical equatio. (b) Calculate the molar concentration of nitric acid 20.00 mL (c) Calculate the pH of the acid. 1.06 mL 23.08 mL

What is the concentration (in molarity) of a solution of HCI of unknown concentration when 24.88 mL of acid is titrated to the end point with 21.19 mL of a 0.189 M NAOH solution.

A student mixes an aqueous solution of ammonium chromate and an aqueous solution of lead (II) nitrate and notices a precipitation form. Write the net ionic equation.

An analytical chemist weighs out 0.151 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0900 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 19.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol

An analytical chemist weighs out 0.087 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1100 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 11.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol Explanation JAYE A @@ W Recheck > # 3 E 80 F3 $ 4 X 8.88 F4 R S C % 5 F5 T 6 MacBook Air Y & 7 4 F7 U * © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 8 DII ( 9 DD O O F10 P ?圖 □ 留 m F11 olo Ar (9)

Part 1 of 2 To a flask, 15.0 mL of 1.25 M HF is added. Then, 3.05 M NaOH is used to titrate the acid sample. Write the balanced net ionic equation for the acid- base reaction. Be sure to include states of matter. Part 2 of 2 00 X 00 ローロ X 3 To determine the concentration of a sample of Ca(OH)2, 1.45 M HCl is added drop-wise using a buret. Write the balanced net ionic equation for the acid- base reaction. Be sure to include states of matter. 0-0 h S