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A 21.428 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is...
A 22.209 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is...
A 22.209 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 80.511 g of water. A 13.858 g aliquot of this solution is then titrated with 0.1069 M HCl. It required 32.29 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste. wt% NH3= %
25.247 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is aluted...
25.247 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is aluted with 72.054 g of water. A 11.243 g aliquot of this solution is then titrated with 0.1076 M HCI. It required 32.33 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste. Number wt% NH,-
A 24.116 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is...
A 24.116 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 73.742 g of water. A 10.766 g aliquot of this solution is then titrated with 0.1083 M HCl. It required 30.63 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste.
A 25.863 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is...
A 25.863 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 74.612 g of water. A 14.159 g aliquot of this solution is then titrated with 0.1059 M HCl. It required 31.31 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste.
A 25.454 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is...
A 25.454 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 75.695 g of water. A 13.872 g aliquot of this solution is then titrated with 0.1053 M HCI. It required 29.89 ml of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste Number 0 0
(1). 500.0 mL of 0.110 M NaOH is added to 535 mL of 0.250 M weak...
(1). 500.0 mL of 0.110 M NaOH is added to 535 mL of 0.250 M weak acid (Ka = 6.08 × 10-5). What is the pH of the resulting buffer? HA(aq) + OH-(aq) = H2O(l) + A- (aq) (2). A 25.863 g sample of aqueous waste leaving a fertilizer )manufacturer contains ammonia. The sample is diluted with 74.612 g of water. A 14.159 g aliquot of this solution is then titrated with 0.1059 M HCl. It required 31.31 mL of...
A 1.00 g pill contains morphine (M = 285.34), a monobasic compound whose conjugate acid has...
A 1.00 g pill contains morphine (M = 285.34), a monobasic compound whose conjugate acid has pKa = 8.21, in addition to an unknown amount of inert material. To analyze the morphine content of the pill, it is dissolved in 50.0 mL 0.1000 M aqueous HCl and the unreacted acid in the resulting solution back-titrated with 0.1000 M NaOH. Which of the following statements about this experiment are correct? I. If the pill contains only morphine, the titration will require...
A 10.00-g sample that contains an analyte is transferred to a 250-mL volumetric flask and diluted...
A 10.00-g sample that contains an analyte is transferred to a 250-mL volumetric flask and diluted to volume. When a 10.00 mL aliquot of the resulting solution is diluted to 25 ml it gives a signal of 0.235 (arbitrary units). A second 10.00 mL portion of the solution is spiked with 10.00 mL of a 1.00-ppm standard solution of the analyze and diluted to 25.00 mL. The signal for the spiked sample is 0.502. Calculate the weight percent of analyte...
please write properly,asking 2.times 3) 2.413 g sample contains Na CO2, NaHCO, and inert material. This...
please write properly,asking
2.times
3) 2.413 g sample contains Na CO2, NaHCO, and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCI was consumed. Calculate the percentage of NaHCO, and Na...
5. To make a saturated aqueous solution of ammonia, 470 g of ammonia are dissolved with...
5. To make a saturated aqueous solution of ammonia, 470 g of ammonia are dissolved with one liter of water. The density of the resulting solution is 0.89 g/mL. What is the molarity of the solution? Hint: Think about the two quantities you need to calculate the molarity of a solution, then figure out how to get those two quantities from the information supplied in the problem, so that you can calculate the molarity. 6. You found a 1 pound...
25.247 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is aluted with 72.054 g of water. A 11.243 g aliquot of this solution is then titrated with 0.1076 M HCI. It required 32.33 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste. Number wt% NH,-
A 25.454 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 75.695 g of water. A 13.872 g aliquot of this solution is then titrated with 0.1053 M HCI. It required 29.89 ml of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste Number 0 0
please write properly,asking
2.times
3) 2.413 g sample contains Na CO2, NaHCO, and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCI was consumed. Calculate the percentage of NaHCO, and Na...
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