You have Falcon tubes containing 10 ml and you should add ,that you have in a voltage series, from which concentration in the dilution series you should pipette 0.1 ml to reach the final concentration of 10-5M in the organ bath Group of response options 10-5M 10-4M 10-3M 10-2M
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You have Falcon tubes containing 10 ml and you should add ,that you have in a voltage series, from which concentration in the dilution series you should pipette 0.1 ml to reach the final concentration of 10-5M in the organ bath
Group of response options
10-5M
10-4M
10-3M
10-2M
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- PS. Further values required for the solvings are give in the various situations below. (ANSWER) Situation: A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Required: SHOW YOUR COMPLETE CALCULATIONS. BASED ON THE IMAGE PROVIDED BELOW FOR THIS QUESTION: Calculate the amount of titrant used in each trial to reach endpoint. Report total hardness of the sample as mean ±sd. a. 250.0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only). Answer : Mass of CaCO3 = 0.125 g b, The EDTA solution was standardized by titrating it with a 25.0 mL aliquot of the CaCO3 solution. How much of the titrant was consumed. Answer: Volume of EDTA consumed = 12.405 g c. Calculate the average titer (mg CaCO3/mL EDTA). Mass of CaCO3 in 25 mL CaCO3 solution: 0.0125 g Answer: 1.008 mg CaCO3/ mL EDTAThe water hardness of tap water has been determined to be 120 (= 120 mg CaCO3 per 1 L of water). After the tap water has run through the ion exchange column, titration of a 20.00 mL sample used only 0.70 mL of 0.0100 M EDTA, to reach the endpoint. Calculate the effectiveness of the ion exchange column: what is the % of the calcium, removed by the ion exchange column? Provide your answer in % and without decimal. ( Please type answer note write by hend)00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M. Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH. Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL 0.1506 M 0.0753 M 0.0376 M 0.1431 M 0.0526 M
- SCE students measured the concentration of HCl in a solution by titrating with different indicators to find the end point.Indicator Mean HCl concentration (M)(± standard deviation)Number of measurementsBromothymol blue 0.09565 ± 0.00225 28Methyl red 0.08686 ± 0.00098 18Bromocresol green 0.08641 ± 0.00113 29Is the difference between indicators 1 and 2 significant at the 95% confidence level? Answer the same question for indicators 2 and 3A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanationIf pH (± 0.5 pH units) strips were used to determine the equivalence point at pH=8.5. What is the relative error (%) in pH at the equivalence point? I assumed it should be 0.5/8.5 * 100 = 5.88, rounded to 5.9 for sig figs. but I got the answer wrong. Please help and let me know how to solve this.
- Can you please please please not reject this question. I really need to know this. AND THIS IS NOT A GRADED QUESTION. So can someone please answer this without rejecting this everytime. I really need to learn how to do the calculations for this becuse I have my exam within 2 weeks. So please someone and this is not a graded question. Okay this time I have included all the information. Molarity is included. An experiment was conducted by following the procedure below. Prepare a 50-mL burette for titration. Rinse the clean burette and tip with two 5-mL portions of standardized 0.005 M HCl solution and discard. Fill the burette with standardized HCl, remove the air bubbles in the tip, and record the initial volume (± 0.01mL). Record the molarity of the HCl solution, which is 0.005M Cover the flask with parafilm to avoid contact with carbondioxide from air. Rinse a 25 mL pipet with 1 or 2 mL of the saturated Ca(OH)2 solution and discard. Pipet 25 mL of the filtrate into a clean…Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Measured mass of the precipitate Question 4 Overignition which causes the conversion of BaSO4 precipitate to BaO. EX ___ ET Question 5 Precipitate was not washed thoroughly. Ex ___ ET TOPIC: Standardization of Titrant Question 6 Adding insufficient amount of titrant to reach acceptable endpoint color: EX ___ ETData Table for Weak Acid Vol. of Titrant pH Avg. Vol. ∆pH/∆vol 0 2.881 0.25 0.622575 0.5 3.193 0.75 0.453769 1 3.420 1.25 0.32668 1.5 3.583 1.75 0.251434 2 3.709 2.25 0.20456 2.5 3.811 2.75 0.173202 3 3.897 3.25 0.150977 3.5 3.973 3.75 0.134517 4 4.040 4.25 0.12191 4.5 4.101 4.75 0.112002 5 4.157 5.25 0.104057 5.5 4.209 5.75 0.097586 6 4.258 6.25 0.092253 6.5 4.304 6.75 0.087819 7 4.348 7.25 0.084111 7.5 4.390 7.75 0.081001 8 4.431 8.25 0.078391 8.5 4.470 8.75 0.076209 9 4.508 9.25 0.074397 9.5 4.545 9.75 0.072912 10 4.582 10.25 0.071719 10.5 4.617 10.75 0.070794 11 4.653 11.25 0.070117 11.5 4.688 11.75 0.069675 12 4.723 12.25 0.06946 12.5 4.757 12.75 0.069467 13 4.792 13.25 0.069696 13.5 4.827 13.75 0.070152 14 4.862 14.25 0.070845 14.5 4.897 14.75 0.071787 15 4.933 15.25 0.072999 15.5 4.970 15.75 0.074507 16 5.007 16.25 0.076346 16.5 5.045 16.75 0.078561 17 5.085 17.25 0.081211 17.5 5.125 17.75 0.084372 18…
- 1. is pH scales is strictly btw 0 and 14? if not, why? 2. what is CSTR? is this heterogenous? is this concentration depends on location? 3. is steady state, mass can enter ot not? leave the control volume or not?A solution of Ca(OH)2 (FM = 74.09) was used in determining the equivalent weight of an unknown acid. To do so, the said solution was standardized against 0.1235 g KHP (FM = 204.22), requiring 7.45 mL to reach the phenolphthalein endpoint. On the other hand, a 0.0543 g unknown acid requires 12.85 mL standard Ca(OH)2 to reach the desired endpoint.a. Calculate the standard normality of Ca(OH)2.b. Calculate the equivalent weight of the unknown acid.c. From the information in the table, what is the most probable identity of the unknown acid?This has got to be one of the worst explanations. No following at all, tried it on a problem 4 different times following the forumla and such and it sucked.
