initial concentration of KIO3 = 0.00364 M
Explanation
Total volume = 20.0 mL + 10.0 mL + 80.0 mL = 110.0 ml
According to dilution law, C1 * V1 = C2 * V2
C1 = concentration before mixing = 0.0200 M
V1 = volume before mixing = 20.0 mL
C2 = concentration after mixing
V2 = volume after mixing = 110.0 mL
C2 = C1 * (V1 / V2)
C2 = 0.0200 M * (20.0 mL / 110.0 mL)
C2 = 0.0200 M * (0.182)
C2 = 0.00364 M
You use 20.0 mL of solution A, 10.0 mL of solution B, and 80.0 mL of...
20.0 mL of a 0.750 M solution is diluted to 80.0 mL. Then, 40.0 mL of this new solution is diluted to 250 mL. Finally, 25.0 mL of this solution is diluted to 175 mL. What is the concentration in moles per liter of the final solution?
A solution is prepared by adding 20.0 mL of 0.15 M HCl to 80.0 mL of 0.20 M NH3. Ka(NH4+)= 5.8 x 10-10 a. Is this solution a buffer? Why or why not? b. What is the pH of the solution?
If you add together 10.0 ml of 0.020 M FeCl3 and 20.0 ml of 0.020 M KI in a beaker what is the initial molar concentration of the KI before the reaction occurs?
In an ethylene glycol-water solution, there are 20.0 g ethylene glycol for every 80.0 g water. This solution is used for filling a 450.0 gallon reservoir. Suppose the density of this mixture solution is ρ= 1.0529 g/ml. (a) What is the molarity of this solution? (b) If you need to fill the 450.0 gallon tank in 170.0 s, what is the volumetric flow rate of the solution into the tank? (c) How many moles of ethylene glycol are in the...
A buffer solution is made by adding 20.0 mL of a 0.50 M Na2CO3 solution to 10.0 mL of a 0.50 M NaHCO3 solution in a test tube. The pH of this buffer was found to be 10.20. After 2.0 mL of 1.0 M HCl solution is added to this buffer solution, the pH is measured to be 9.95. What is the buffering capacity with respect to a strong acid, βa, of this buffer solution, in units of mol/L per pH unit?...
I just wanted to check if my answers were correct for the initial concentrations of mixture 4 #7-9. DATA & RESULTS When the lab was performed as described in your lab manual, the following times were recorded for each mixture to change from pale yellow to clear: Mix acetone HCI lodine water Time, 1 trial Time, 2 trial Temp 1 10.0 mL 10.0 mL 10.0 ml 20.0 ml 290 294 24.1°C 2 200 ml 10.0 mL 100 ml 10.0 ml...
O STOICHIOMETRY Dilution A chemist makes 80.0 ml. of potassium dichromate (K,Cr,0,) working solution by adding distilled water to 60.0 ml. of a 0.0763 M stock solution potassium dichromate in water. Calculate the concentration of the chemist's working solution. Be sure your answer has the correct number of significant digits 다,p
A solution is prepared by mixing 20.0 mL of 0.050 M acetic acid and 10.0 mL of 0.100 M HCl. What is the pH of the solution? ( Ka acetic acid = 1.8 x 10-5) A. 2.36 B. 0.22 C. 1.48 D. 1.00 E. 0.48
You need 100 mL of a 0.00057 M solution for an experiment. You are given 10 mL of a 5.7 M stock solution. What is the best method to get the final volume and concentration you for trial? -It is not possible to reach that concentration with the info presented. -Use a 1.0 mL volumetric pipette and then dilute with water to 100 mL, then repeat serially until the desired concentration is reached. -Use a graduated cylinder to measure 0.1...
If a mixture was prepared by diluting 7.0 mL of the Blue#1 solution with water to a final volume of 10.0 mL and mixing this with 2.0 mL of diluted bleach how many seconds would it require for the mixture to have an absorbance of 0.120? Use your measured values of eb and of the average rate constant, k to answer this question. Show all work. eb= 0.1138 k= -0.035 first order reaction Concentration of Blue Solution= 15 M