you have a mixture of acids and bases at the following concentrations [Mg (OH) 2] =...
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have a mixture of acids and bases at the following concentrations
[Mg (OH) 2] =...
Consider the following data on some weak acids and weak bases: acid Ka name formula nitrous...
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...
Consider the following data on some weak acids and weak bases acid base name formula name...
Consider the following data on some weak acids and weak bases acid base name formula name formula hydrocyanic acid| HON|49-10-101 lammonial NH3 | 1.8×10-5 nitrous acid HNO2 4.5 104aniline CHNH2 4.3 10-10 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 ? next to the solution that will have the next lowest pH, and so on. solution PH 0.1...
Consider the following data on some weak acids and weak bases: acid base Ka Кь name...
Consider the following data on some weak acids and weak bases: acid base Ka Кь name formula name formula -4 hydrofluoric acid HF 6.8 x 10 ammonia NHZ -5 1.8 x 10 4 HNO2 4.5 x 10 -4 nitrous acid ethylamine C2H5NH2 6.4 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution...
Consider the following data on some weak acids and weak bases: acid base K. - K...
Consider the following data on some weak acids and weak bases: acid base K. - K name formula name formula hydrofluoric acid HF 16.8 x 10-4 methylamine CH3NH2 4.4 x 10-4 ammonia NH3 1.8x10-5 nitrous acid HNO2 4.5 x 10-4 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next...
Consider the following data on some weak acids and weak bases: acid Кр name formula base...
Consider the following data on some weak acids and weak bases: acid Кр name formula base name formula hydroxylamine HONH2 1.1 x 10-8 hypochlorous acid HCIO 3.0 x 10-8 hydrofluoric acid HF 6.8 x 10-4 ammonia NH3 | 1.8 x10-5 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
The following shows a list of weak acids and bases with their Ka and Kb values....
The following shows a list of weak acids and bases with their Ka and Kb values. Substances Ka Substances Kb Cyanic acid (HCN) 4.9 x 10-10 Ammonia (NH3) 1.8 x 10-5 Nitrous acid (HNO2) 4.5 x 10-4 Aniline (C6H5NH2) 4.3 x 10-10 Hydrofluoric acid (HF) 6.8 x 10-4 Pyridine (C5H5N) 1.7 x 10-9 Acetic acid (CH3COOH) 1.8 x 10-5 Methylamine (CH3NH2) 4.4 x 10-4 If you want to make a pH 8.0 buffer solution, which of the following acids or...
3. i). Write the formula of four strong acids and four strong bases. ii). List four...
3. i). Write the formula of four strong acids and four strong bases. ii). List four factors that affect the strength of an acid. iii). Predict the relative strength of the following compounds: H2O, H2S and H2Se. iv). Which of the following is the stronger acids: CHCICOOH or CHCI-COOH? Explain. v). Al 3* is not a Bronsted acid, Al(H2O)" is. Explain. vi). All Bronsted acids are Lewis acids, but the reverse is not true. Give two examples of two Lewis...
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2?...
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Ksp = 1.5x10-11) b. If NH3/NH4+ buffer is used to control the pH, and [NH3] = 0.10 M, what concentration of NH4 is required to prevent the precipitation of Mg(OH)2?
PROBLEMS 1) Acids and bases: Calculate the following a) [H30] in a 0.500 M solution of...
PROBLEMS 1) Acids and bases: Calculate the following a) [H30] in a 0.500 M solution of HCl b) pH of a 0.100 M solution of HCI c) pH of a 0.100 M solution of HNO3 d) [OH] in a 0.500 M solution of HClnote, for this you need to use Kw e) pH of a 0.100 solution of NaOH (also need to use some form of Kw here)
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...
Consider the following data on some weak acids and weak bases acid base name formula name formula hydrocyanic acid| HON|49-10-101 lammonial NH3 | 1.8×10-5 nitrous acid HNO2 4.5 104aniline CHNH2 4.3 10-10 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 ? next to the solution that will have the next lowest pH, and so on. solution PH 0.1...
Consider the following data on some weak acids and weak bases: acid base Ka Кь name formula name formula -4 hydrofluoric acid HF 6.8 x 10 ammonia NHZ -5 1.8 x 10 4 HNO2 4.5 x 10 -4 nitrous acid ethylamine C2H5NH2 6.4 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution...
Consider the following data on some weak acids and weak bases: acid base K. - K name formula name formula hydrofluoric acid HF 16.8 x 10-4 methylamine CH3NH2 4.4 x 10-4 ammonia NH3 1.8x10-5 nitrous acid HNO2 4.5 x 10-4 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next...
Consider the following data on some weak acids and weak bases: acid Кр name formula base name formula hydroxylamine HONH2 1.1 x 10-8 hypochlorous acid HCIO 3.0 x 10-8 hydrofluoric acid HF 6.8 x 10-4 ammonia NH3 | 1.8 x10-5 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next...
3. i). Write the formula of four strong acids and four strong bases. ii). List four factors that affect the strength of an acid. iii). Predict the relative strength of the following compounds: H2O, H2S and H2Se. iv). Which of the following is the stronger acids: CHCICOOH or CHCI-COOH? Explain. v). Al 3* is not a Bronsted acid, Al(H2O)" is. Explain. vi). All Bronsted acids are Lewis acids, but the reverse is not true. Give two examples of two Lewis...
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Ksp = 1.5x10-11) b. If NH3/NH4+ buffer is used to control the pH, and [NH3] = 0.10 M, what concentration of NH4 is required to prevent the precipitation of Mg(OH)2?
PROBLEMS 1) Acids and bases: Calculate the following a) [H30] in a 0.500 M solution of HCl b) pH of a 0.100 M solution of HCI c) pH of a 0.100 M solution of HNO3 d) [OH] in a 0.500 M solution of HClnote, for this you need to use Kw e) pH of a 0.100 solution of NaOH (also need to use some form of Kw here)
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