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sangriagnu673Lv1

28 Nov 2020

The label on a bottle of organic liquid fertilizer concentrate states that it contains 8.4 grams of phosphate per 100 mL and that 16 fluid ounces should be diluted with water to make 32 gallons of fertilizer to be applied to growing plants. What is the phosphate concentration in grams per liter in the diluted fertilizer? (1 gallon = 128 fluid ounces)

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Bryllant BaluyutLv10

21 Jan 2021

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The label on a bottle of "organic" liquid fertilizer concentrate states that it contains 7.40 grams of phosphate per 100.0 mL and that 16.0 fluid ounces should be diluted with water to make 32.0 gallons of fertilizer to be applied to growing plants. What version of the dilution equation can be used to calculate the final phosphate concentration? Express your answer in terms of Vi, Ci, and Vf.

If someone could help me solve the first column of trial #1, I just need to see the steps to solve and then I can finish the rest. Thank you!

The solubility of Borax equal to the number of moles of The number of moles of Borate ions produced in solution is the solubility of solid Borax that dissolved, therefore the concentration of Borate ions is equal to Borax in water. that of borateton Note that the sodium theoquilibrium solution calculate the concentration. By finding the borate ion concentration experimentally you can casily Reaction 2. corresponding sodium ion concentration, and therefore the equilibrium constant for PROCEDURE PREPARATION OF BORAX-BORATE EQUILIBRIUM MIXTURES 1. Room Temperature Solution: Add 3 grams of solid borax, 50 mLofdistilled water and a stir bar to a 100-mL beaker Place on a magnetic stirrer and stir the mixture for at least 15 If minutes. Periodically stop the stirring and make sure there is undissolved borax present. not add some more borax There must be undissolv boraxpresent in order to have 2. equilibrium. Why? a stir Ice Bath Temperature solution: Add 3 grams of solid borax 50 mL of distilled water and a second 100-mL Place this beaker in an ice-water bath and place the bath on magnetic stir for 25-30 minutes. As above, check to make sure there is undissolved stirrer and borax present and add more if necessary. Borate on is weak base o can be titrated with a sandardized hydrochloric acid solution according to Reaction 3 (3) or more simply (4) Note that it requires 2 moles of hydrochloric acid per mole of borate ion for the titration. 3. The HCI solution has been prepared for you by the stockroom. It should be approximately 0.2 M, however, on your data sheet you will need to record the exact molarity of the HCI solution as given on the bottle. 4. Prepare the Buret: Pour approximately 70 to 80 mL of the standard (0.2 M) HCI solu tion into a 250 ml beaker. Record its molarity on your repolt sheet. Clean a 50-mL buret, rinse it with 5-10 mL of HCI solution and let drain. Close the stopcock and fill the buret with the HCI solution. Finding Kspr Titrating Room Temperature Borax with HCI Laboratory 7 l Finding Equilibrium Constants: The solubility of Borax 97

You need a strong acid for an experiment, and you are given a bottle that you are told contains a strong acid at 15.0 M concentration. (The name of the acid on the label was rubbed off, so you are not sure of the identity of the acid.) You make a 0.1 M solution and you want to know if you can assume that the [H+] will be 0.1 M since the acid is a strong acid and thus should (so you have been told) completely dissociate. You see that the label on the bottle lists a pKa for the acid of -6.5. A pKa? Why does a strong acid have a pKa? You decide that you better calculate the relative error that will result when you make the assumption that a 0.1 M solution of the strong acid will result in a 0.1 M [H+] versus the concentration that you obtain when you properly treat the dissociation using the listed pKavalue. Normally, the relative error is expressed as follows: Er = ((xi â xt)/xt) Ã 100; where xi is the value under the assumption that complete dissociation occurs and xt is the true or actual value obtained when the pKa of the acid is taken into account. Now, the units for an answer that is expressed as a percent could equivalently be stated as âparts per hundredâ. Because the value of ((xi â xt)/xt) is likely to be a small number, I want you to multiply this value by 109 rather than 102 (as shown in the above equation). Thus, your answer will be in terms of parts per billion (ppb), and you should report your answer in these terms to the nearest ones (e.g., enter â11â if your answer is 11 ppb). For this problem, you can ignore the contribution of H+ ions due to the autoproteolysis of water. You will need to do this problem with the aid of a spreadsheet, and be sure to adjust the format of the cells to retain several figures beyond the decimal point.

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