ubjected to pH analysis using a pH meter, the first is analysed using 1:1 soil:water ratio and the other with 1:1 soil:KCl ratio, what would be the most probable result
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- 1.Two samples of the same soil is subjected to pH analysis using a pH meter, the first is analysed using 1:1 soil:water ratio and the other with 1:1 soil:KCl ratio, what would be the most probable result? a. Soil analysed using 1:1 soil:water ratio will register a lower pH compared to that of soil analysed using 1:1 soil:KCl ratio b. Soil analysed using 1:1 soil:water ratio will have the same pH with that of soil analysed using 1:1 soil:KCl ratio c. Soil analused using 1:1 soil:KCl ratio will register a higher pH compared to that of soil analysed using 1:1 soil water ratio d. Soil analysed using 1:1 soil:KCl will register a lower pH compared to that of soil analysed using 1:1 soil:water ratio 2. when a soil whose exchange sites were saturated with H+ is tested for pH using a litmus paper, what is the most probable result? a. red litmus paper manifests a false positive b. Red litmus paper turns blue c. Blue litmus paper turns red d. blue litmus paper manifests a false positive 3.…9. wo samples of the same soil is subjected to pH analysis using a pH meter, the first is analysed using 1:1 soil:water ratio and the other with 1:1 soil:KCl ratio, what would be the most probable result? A. Soil analused using 1:1 soil:KCl ratio will register a higher pH compared to that of soil analysed using 1:1 soil water ratio B. Soil analysed using 1:1 soil:KCl will register a lower pH compared to that of soil analysed using 1:1 soil:water ratio C. Soil analysed using 1:1 soil:water ratio will register a lower pH compared to that of soil analysed using 1:1 soil:KCl ratio D. Soil analysed using 1:1 soil:water ratio will have the same pH with that of soil analysed using 1:1 soil:KCl ratioTable 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 49.32 49.06 49.93 Table 2. Titration data Table view List view Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 49.32 49.06 49.93 Expected color at end point Choose... Choose... Choose... Volume of NaOH used (mL) 1. Average Volume of NaOH used in liters 2. Average moles of NaOH used (mol) 3. Average moles of acetic acid (mol) 4. Average molarity of acetic acid (M) 5. Average mass of acetic acid (g)…
- 4.What will be the change in pH after adding 13.4ml of the titrant? * Present your answer to the 2ⁿᵈ decimal place 5.What will be the change in pH after adding 26 ml of the titrant? Present your answer to the 2ⁿᵈ decimal place 6.What is the total volume at equivalence point? Present your answer to the 2ⁿᵈ decimal place 7.What is the pH at equivalence point? Present your answer to the 2ⁿᵈ decimal place 8.Upload a clear and well-lit image of a hand-written, completely plotted and labeled titration curve .A solution of acetic acid has pH = 3.5. A small portion of sodium hydroxide (NaOH) is added to the acetic acid solution to make a new solution. Say if the following statement is TRUE or FALSE: After the addition of the NaOH the pH of the new solution will be greater than 3.5. A. True B. FalsWrite the Henderson-Hasselbalch equation for a propanoic acid solution (CH, CH, CO, H, pK, = 4.874). + log Answer Bank pH pK [A] [HA] Using the equation to calculate the quotient [A /[HA] at three different pH values. [A ] [HA] pH = 4.373 [A] pH = 4.874 [HA] [A] [HA] pH = 5.186
- 1. What is the ratio of water drops to EDTA if 2 drops of EDTA is needed to change the color of 20 drops of water with unknown hardness? A. 10B. 5C. 0.1D. 1.0 2. The higher the value of chemical oxygen demand indicates the higher organic pollution in the water sample. A. True B. False 3. COD measures the total amount of O2 needed to oxidize all organic matter into CO2 and water. A. True B. FalseThank you! Data included in picture! No hand drawn graphs!! Determine the equivalence point of sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 1: No Indicator Data Table. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration in Part 4. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental solution at that volume. Do NOT connect your points; no trend line needed and make sure to: · Label the axes including the units in parentheses. · Include a figure legend (text below the graph) explaining the data in your graph that includes the arrow…Saved CHEMY 101 SEC SEM T2 2020-21 The amount of water which should be added to 0.700 M NAOH solution to make 100 mL 0.250 M solution is 19 Multiple Choice 01:25:58 79.6 mL 35.7 mL 55.2 mL 64.3 mL raw K Prev 19 of 20 Next >
- Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.55 49.43 49.99 Expected color at end point Volume of NaOH used (mL) Average Volume of NaOH used in liters Average moles of NaOH used (mol) Average moles of acetic acid (mol) Average molarity of acetic acid (M) Average mass of acetic acid (g) Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL) Average mass % of acetic acid in vinegar Known mass % of acetic acid in vinegar is 5.45% Percent ErrorB. Molar Concentration of an Acid Solution Acid type, HA or H,A: HA Unknown No. Balanced equation for neutralization of acid with NaOH. NaOH + HCI = NaCI + Sample 1 Sample 2 Sample 3 1. Volume of acid solution (mL) 25.0 25.0 25.0 2. Buret reading of NaOH, initial (mL) 0.00 0.00 0.00 3. Buret reading of NaOH, final (mL) 26.3 26.0 26.8 26.3 26.0 0.148 4. Volume of NaOH dispensed (mL) 26.8 5. Molar concentration of NAOH (mol/L), Part A 6. Moles of NaOH dispensed (mol) 7. Molar concentration of acid solution (mol/L) 8. Average molar concentration of acid solution (mol/L) Data Analysis, B 9. Standard deviation of molar concentration Data Analysis, C 10. Relative standard deviation of molar concentration (%RSD) Data Analysis, DTitration Experiment 1: Acid-Base Titration: Unknown HCl Write chemical equation *+ HClcags N s → Naclceg) + H,O Write NIE OH c) + HEogs → H2OC) Enter the data into the table and choose three titrations to find the molarity of the unknown HCI. Unknown # HCI Titration 1 Titration 2 Titration 3 Titration 4 Titration 5 Volume NaOH used to titrate unknown HCI solution 17.43ml 16.5O ml662 mll16.57ml16.6dmL Molarity of NaOH used for each titration 0.2564 0.1787/01692/0.1704/oiado1703 Molarity of HCI Average M HCI (avg ± standard deviation) 10.1717 1.63 % Precision Calculations 1. Provide one representative calculation that you used to determine the molarity of HCI. Be sure to show all units and use proper sig figs! V HCI-25mL MHCI =? VN2OH = 16.6lmL MNAOH=0.2564 MHCI VHCI=MNAOH VAa OH MHCI 25=O. 1564 16.61 MHCI= 0.2564.16.61 25 MHCI=0.1703 2. Average molarity of three titrations. 6.1787+0.1692+0.1704+0.1619+ O.1703 MACI= 0.117
