Sort the following 0.1 M solutions in order of increasing
pH
? ? NaCl ? NH4Cl ? NaNO2 ? NaCN
Ka(HCN) = 6.2 x 10-10 ? Ka(HNO2) = 7.2 x 10-4 ? Kb(NH3) = 1.8 x
10-5
Sort the following 0.1 M solutions in order of increasing pH ? ? NaCl ? NH4Cl...
Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO, HCl, HCN, NaOH, NH3, NaCN, KNO3, H2SO4, NH4Cl, H2SO3, NaHCO3, Na3PO4 and CH3COOH. please list each solution in order and next to it be specific next to each in terms of why each solution was placed in its respective position - please include ka and kb values in your explanation while ranking the solutions and add in any...
Which of the following combinations would make a buffer with pH close to 3.0? HClO2 Ka = 1.1 × 10-2 NH3 Kb = 1.8 × 10-5 HNO2 Ka = 7.2 × 10-4 C5H5N Kb = 1.5 × 10-9 Equal volumes of 0.10 M NH4Cl and 0.10 M NH3 Equal volumes of 0.10 M HClO2 and 0.10 M NaClO2 Equal volumes of 0.10 M HNO2 and 0.10 M NaNO2 Equal volumes of 0.10 M HCl and 0.10 M NaCl Equal volumes...
1.) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl 200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M HF (Ka = 7.2 x 10-4) by 0.100 M NaOH 100.0 mL of 0.100 M HCl by 0.100 M NaOH...
1) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M KOH by 0.100 M HCl 200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M NH3 (Kb = 1.8 x1 0-5) by 0.100 M HCl 100.0 mL of 0.100 M HI by 0.100 M NaOH 100.0 mL of 0.100 M...
Rank the following solutions in order of increasing pH. Consider the following data on some weak acids and weak bases: - Ka Ko acid name formula nitrous acid HNO2 4.5*10-4 base name formula methylamine CH3NH2 4.4 x 10-4 acetic acid HCH,CO2 1.8 x 10-5 aniline CH3NH2 4.3 * 10-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the so the solution that will have the next lowest...
Which one of the following solutions has the lowest pH? A. a 0.1 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) B. a 0.1 M solution of ammonium chloride, NH4Cl(s) (Ka (NH4+) = 5.6 x 10-10) C. a 0.01 M solution of acetic acid, CH3COOH (Ka = 1.8 x 10-5) D. a 0.01 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) E. a 0.1 M solution of acetic acid, CH3COOH (Ka = 1.8 x...
Consider the following data on some weak acids and weak bases: acid Ka name formula nitrous acid HNO2 ×4.510−4 acetic acid HCH3CO2 ×1.810−5 base Kb name formula ammonia NH3 ×1.810−5 ethylamine C2H5NH2 ×6.410−4 Use this data to rank the following solutions in order of increasing pH. In other words, select a ' 1 ' next to the solution that will have the lowest pH, a ' 2 ' next to the solution that will have the next lowest pH, and...
Rank the following titrations in order of increasing pH at the equivalence point of the titration (1 = lowest pH and 5 = highest pH). 1 2 3 4 5 100.0 mL of 0.100 M HNO2 (Ka = 4.0 x 10-4) by 0.100 M NaOH 1 2 3 4 5 100.0 mL of 0.100 M HOCl (Ka = 3.5 x 10-8) by 0.100 M NaOH 1 2 3 4 5 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100...
20. If 10 mL of 0.05 M NaOH is added to a 20 mL solution of 0.1 M NaNO2 and 0.1 M HNO2, what will be the pH of the resultant solution? Assume that volumes are additive. Ka for HNO2 = 7.1x10-4. 21. At 25°C, 50.0 mL of 0.50 M NaOH(aq) is added to a 250 mL aqueous solution containing 0.30 M NH3 and 0.36 M NH4Cl. What is the pH of the solution after the addition of the base?...
Which of the following 1.0 M solutions would have the lowest pH? Weak Base Weak Weink Ka Kb Acid HCN 4.9 x 10-10 HONH2 1.1 x 10-8 A) LINO3 HNO2 4.5 x 10-4 NH3 1.8 x 10-5 B) HONH3Br HIO 2.3 x 10-11 C6H5NH2 4.3 x 10-10 C) H2NNH3CIO4 HBrO 2.5 x 10-9 H2NNH2 1.3 x 10-6 D) Ca(Bro)2 CoH5COOH 6.3 x 10-5 C5H5N 1.7 x 10-9