c 0 0
c - cα cα cα
ct = c - cα + cα + cα = c + cα
α = 0.647
ct = 0.149
0.149 = c + c(0.647)
1.647c = 0.149
c = 0.149/1.647 = 0.09
[H+] = cα = 0.09 * 0.647 = 0.5823
[A-] = 0.5823 =cα
pH = -log[H+] = -log 0.5823 = 1.235
This question has multiple parts. Work all the parts to get the most points. Supply the...
Calculate the concentrations of H, 0* OH, HSO," and Seo, in 0.12MH, Sesselenic acid, solution (This problem requires values in your textbook's specific appendices, which you can access through the OWL 2 Mind Tap Reader. You should not use the OWLV2 References Tables to answer this question as the values will not match.) Concentration of 1,0 - M Concentration of OH- M Concentration of HSO- M Concentration of Seo M Very large =K1 1.92 1.2 x 10-2 Ka2
Calculate the pH of 1.2M solutions of the following salts: (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a. NaNO2 PH- b. KOCI pH- c. LiCsHsO pH- Submit Answer 3 question attempts remaining
Calculate the pH of 1.2M solutions of the following salts: (This problem requires values in your textbook's specific appendices,...
Calculate the molar solubility of BaSO4 in a solution in which H307 (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) @ 4.5 M. Molar solubility = b 0.8 M Molar solubility = C 0.076 M. Molar solubility = M d 0.260 M. Solubility =
A buffered solution is made by adding 80.08 NH, Cl to 1.00 L of a 0.65-M solution of NH, Calculate the pH of the final solution (Assume no volume change.) (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 Mind Top Reader. You should not use the OWLv2 References Tables to answer this question as the values will not match.) pl -
17-entropy
Predict the sign of AS and then calculate A5 for each of the following reactions (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 Mind Tap Reader. You should not use the OWLv2 References Tables to answer this question as the valoes will not match.) 1. He(9) +0,6) +7,00 AS is AS- JK b. 2CH, OH(9) +30, (g) 200,(9) + 4H2O(g) AS- JIK HBr(9) H(aq) + Brag) AS is AS = J/K...
What mass of glycerin (C,H,Os), a nonelectrolyte, must be dissolved in 200.0 g water to give a solution with a freezing point of -2.20°C? (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.)
A buffered solution is made by adding 40.0 g NH4 Cl to 1.00 L of a 0.65-M solution of NH3. Calculate the pH of the final solution. (Assume no volume change.) (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) pH =
Calculate the pH of a solution that contains the following analytical concentrations: (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a 0.210 M in H3PO4 and 0.468 M in NaHPO4. b 0.0180 M in Na2SO3 and 0.0368 M in NaHS O3. c 0.460 M in HOC2H4NH2 and 0.840 M in HOC2H4NH3CI. d 0.0110 M in H2C2O4 (oxalic...
My answer(s) were marked as incorrect. My textbook's Ka values
for H3PO4 are: Ka1=7.11x10^-3, Ka2=6.32x10^-8, and
Ka3=4.5x10^-13
What is the pH of the buffer formed by mixing 83.0 mL of 0.280 M Na H2PO4 with (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a. 44.0 mL of 0.470 M HCI? pH =...
Please give the answers in mL.
The Ka value given by my textbook for carbonic acid are:
Ka1=4.45x10^-7 and Ka2=4.69x10^-11.
How would you prepare 1.20 L of a buffer with a pH of 9.35 from 0.200 M Na2CO3 and 0.450 M HCl? (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) Mix mL...