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A: The valid equation for dilution, M1V1=M2V2
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A: Given is, Molarity= 0.069 M Standard value, Molar mass of acetic acid =60.052 g/mol
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A: To solve this problem we will use the formula of dilution law . According to this law M1V1 = M2V2…
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A: • 211.3424 grams of Ca(NO2)2 is needed to make 800. mL of a 2.00 M Ca(NO2)2…
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- To which sample solution the spike will be add? the distillate>130C the mass standard the distilled <130CHello! I need the solution of the question attached. Thanks!Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1) find Ka and use the value of Ka to calculate the initial pH of each trial 2) calculate Kb for the C8H4O4^-2 anion from the value of Ka that you obtained for KHP.
- Hello help w this question the bottom options are (greater) or (less).find the mol Na2S203 delivered for sample 1 and 2 find the mol of IO3- present for sample 1 and 2 find M of IO3- for sample 1 and 2 from the given information in the data tableThe answer for volume NaOH= 22.50ml is ph= 8.651 And i cant figure it out. Pls help
- the ALEKS calculator to find 65% of 45 . Do not round your answer.The Ka value for benzoic acid (C6H5COOH) is 6.3×10^−5 and for phenol (C6H5OH) thevalue of Ka is 1.3×10^−10. Which is a stronger base, C6H5COO− (aq) or C6H5O− (aq)?Explain your answer (write reactions to illustrate).Please find the pH calculation. Kb=1.5•10-12 use ICE table if needed. Result should come out to be about 1.66
- MATLAB The acidity of solutions is generally measured in terms of pH. The pH of a solution is defined as theconcentration of hydronium ions. Create a table of conversions from concentration of hydronium ionto pH, spaced logarithmically from 0.001 to 0.1 mol/liter with 10 values. Assuming that you havenamed the concentration of hydronium ions H_conc, the syntax for calculating the negative of thelogarithm of the concentration (and thus the pH) is:pH = -log10 (H_conc)6 I- + BrO3- + 6 H+ ----- 3 I2 + Br- + 3 H2O Rate= k[I-]m[BrO3-]n[H+]p rate= (∆[I2])/(3*∆time) [I-] 0.010M [S2O3-2] 0.0010M H2O [BrO3-] 0.04M HCl 0.10M Starch Indicator (sec.) Volume, ml Volume, ml Volume, ml Volume, ml Volume, ml 1 10 10 20 10 10 1-3 drops 301.90 2 20 10 10 10 10 1-3 drops 213.28 3 10 10 10 20 10 1-3 drops 214.92 4 10 10 10 10 20 1-3 drops 86.45 Temperature of Reaction: _______20 C________ 1. Using the dilution equation (M1V1 = M2V2) calculate the concentration of the I-, BrO3- and the H+ (HCl) in the final mixture just prior to any reaction. 2. Calculate the rate for each experiment as explained in the background information. 3. Using the information above determine the rate law (m, n and p) for the reaction. Show all calculations/reasoning in your notebook. m_____________ n_________________ p…With using sig figs I came up with the answer of 530mL but I do not feel confident with that answer.