A (aq) + ....B(aq) Č(s)+ D (aq) Experimental Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 3 1.6 9.02 1.8 9.90 2.0 10.86 2.2 10.90 7 2.4 10.88 8. 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph. NM4

A (aq) + ....B(aq) Č(s)+ D (aq) Experimental Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 3 1.6 9.02 1.8 9.90 2.0 10.86 2.2 10.90 7 2.4 10.88 8. 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph. NM4

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

there isn’t a block for .155 … Can you please help line them up exactly in the correct order and exact unit that are in the bank below?
SOLUBILITY CURVES KI 140 130 120 110 100 NONO 90 KNO HCI NH3 70 NH CI 60 KCI 50 40 NaCi- 30 KCIO3 20 O 1O 20 30 40 50 do 7O 80 9o 100 TEMPERATURE C 1. What mass of solute will dissolve in 100 g of water at the following temperatures? a. KNO3 at 70°C b. NaCl at 100°C c. NH&Cl at 90°C d. Which of these 3 substances is most soluble in water at 15°C? %3D GRAMS OF SOLUTE/IO0g MO
7. How many Equivalents are generated for each electrolyte solution? a. 2.0 mole Fe 3+ (aq) b. 2.5 mole SO 2- c. 4.0 mole PO 4 d. 3.5 mole CO. 3- 2- = 3 (aq) = = = 4 (aq) 8. How many mL of a 4.50 M HCl solution are needed to completely react with 20.5 g of CaCO3 if the chemical reaction is as shows below? Hint: use example in Section 9.5 2HC1 + CaCO (aq) 3(s) CaCl + CO 2(aq) 2(g) + H₂OO
Q7) The indicator that is used for Vitamin C analysis is. a) Phenolphthalein b) 1₂ c) Starch d) KI
5 volume of base ..
esc Fr 2 What mass of precipitate is formed when 100. mL of 0.300 M NaCl reacts with 100. mL of 0.150 M Pb(NO3)? Round your answer to 3 significant digits. 55°F Clear 1 F1 B.D F2 @ 2 F3 3 E F4 LA 4 x10 Q Search F5 X % 5 S F6 C A 6 F7 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibil B 8 & 7 F8 * ос F9 DELL prt sc F10 home Submit Assignment F11 A end F12 insert + 5/
In part A of the Experiment, you are asked to prepare three saturated solutions of cadmium oxalate. This is achieved by mixing 0.100M solutions of sodium oxalate and cadmium nitrate together, to form cadmium oxalate. What piece of glassware should be used to measure the desired volumes of the sodium oxalate and cadmium nitrate solutions? A. a 10-mL graduated cylinder B. a buret C. a 50-mL graduated cylinder D. a volumetric pipet
in a stock solution of 5 M base, what volume is needed for the base to titrate with the acid? in each instance? If each acid solution has a concentration of 10 M in a volume of 300 mL, and . Create balanced equations for the reactions between each acid and base. What salt is created w your wOrk. Carry he umts uog" significant figure rules. o 5 a. Hydrochloric acid and calcium carbonate. b. Phosphoric acid and sodium bicarbonate.
Don
! A solid mixture containing MgSO4 is dissolved in water and treated with an excess of Ba(NO3)2, resulting in the precipitation of 0.6 g of BaSO4.The molecular weight of BaSO4 is 233 g/mol. Number of moles of MgSO4 in the mixture is? 0.02570 mol 0.00257mol 0.05720 mol 0.52700 mol 0.25700 mol If the concentration of chloride ion is 1.5xE(-5) then the solubility product of AgCl is--- 2.00x10(-10) 1.69x10(-10) 1.96x10(-10) 0.69x10(-10) 19. x 610(-10)
A. A Set of Standard Solutions Data Analysis, A 16a mmin 16b B. Determination of max Identify the metal ion for analysis on the Report Sheet. 1. Prepare a stock solution. a. Prepare 100 mL of a 0.10 M stock solution. To do this, you will need to know the formula of the Cu²+, Ni²+, or Fe³+ ion-containing salt in order to calculate the mass of salt for its preparation. See Prelaboratory Assign- ment question 2a. Show a similar calculation for your selected metal ion on the Report Sheet. Measure the mass of the salt (±0.001 g). b. Transfer the salt to a 100-mL volumetric flask, half-filled with 0.01 M HNO3, add the appropriate complexing agent (see Table 35.1), and then dilute to the mark with 0.01 M HNO3. Record on the Report Sheet the exact molar concentration of the stock solution. Table 35.1 Volume of Complexing Agent for Stock Solution Preparation Metal Ion Volume of Complexing Agent Cu²+ 10 mL of conc NH, Ni²+ 10 mL of conc NH; Fe³+ 20 mL of 0.1 M NASCN 2. Prepare the standard…
1. Reaction Add 1 drops of … Add 1 drops of… Did a precipitate form? 1 Fe(NO3)3 Na3PO4 2 AgNO3 3 Zn(NO3)2 4 Al(NO3)3 5 Pb(NO3)2