Molarity of stock KMnO4 : (read from bottle in lab) 0.01994 M Volume of KMnO4 Stock Solution added via pipet 5.00ml Calculated Molarity of solution BI

Data is the first picture, questions on the second paper

What volume of 0.0500 M CoCl2 times 6H2O is required to react completely with 75.0 mL of 0.0500 M K3PO4?

G TuT https://app.101edu.co If 24.6 g of KBr (MM = 119.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KBr in the resulting solution? Type here to search F3 K $ Et F5 % n F6 Question 28 of 32 F7 99+ DELL F8 L g & F10

What mass of LiCl is formed from mixing 0.144L of 0.212 molar BaCl2 with 1.22L of 0.0223 molar LiNO3 ?

A 623 mL NaCl solution is diluted to a volume of 1.45 L and a concentration of 4.00 M. What was the initial concentration? Express your answer with the appropriate units. • View Available Hint(s) HA M1 = 8.88 M Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining Review your calculations and make sure you round to 3 significant figures in the last step.

The steps for determining the concentration of a sample of hydrochloric acid are listed below :Step (1): A 0.1038 M standard sodium carbonate solution was prepared by dissolving 2.750 g ofanhydrous sodium carbonate solid in deionised water and made up to 250.0 cm3.Step (2): 25.0 cm' of the standard solution obtained in Step (1) was transferred to a clean conical flask andthen a few drops of methyl orange were added.Step (3): The sample of hydrochloric acid was put into a burette. The standard solution in the conicalflask was titrated with the hydrochloric acid.Step (2) and Step (3) were repeated for several times. The table below shows the results of the titrations:Trial I 2 3 4Final burette reading/ cm330.85 28.75 28.30 31.35 27.25Initial burette reading/ cm32.00 1.50 1.00 3.00 0.00(a) Describe the procedure in preparing the standard sodium carbonate solution in Step (I). (b) State the colour change at the end point of the titration. (c) Calculate a reasonable average for the volume…

Pls help with this chemistry question.

5 volume of base ..

A 35.0 mL volume of ammonia (NH3) household cleaner needs 53.75 mL of 0.300 M HNO3 to completely neutralize the base. The balanced equation is: HNO3 + NH3 --> NH4NO3 A) Find the number of moles of HNO3 involved in this reaction. (2 hints: start dimensional analysis with the volume of HNO3, & convert mL to L.) B) Find the molarity (M) of the NH3 (This is different than the number of moles. Your calculation will be different from part A.) C) Find the mass/mass % of the NH3. You will need the molar mass of NH3 (17.04 g/mol) & the density of NH3 (0.985 g/mL).