Which of the following gives the correct order of increasing strength of the conjugate bases of those acids?
491609
The weaker the acid, the stronger the conjugate base.  The stronger the acid, the weaker the conjugate base.\n\nBy "strong", we are refering to its ability to dissassociate in water and break into ions.\n\nIt might help if you convert all your pKa values to Ka, or all your Ka values to pKa to make it easier to compare.\nWhat does a high Ka value mean?  What does a low Ka value mean?  How does this compare to your definition of a "Strong" acid/base or a "strong" conjugate acid/conjugate base?
468312
Potassium hydroxide is a strong base.\nKOH -> K+ + OH-\n\nWater doesn't participate directly in the reaction, so you can leave out the H2O on both sides. Because KOH is a strong base, it's pretty accurate to just have the arrow pointing one way in the reaction -- almost all of the KOH disassociates. For weak acids and bases, instead of an arrow pointing just in one direction, you need a bidirectional arrow to show that both sides of the equation are present in the solution. For example,\nH2CO3 <---> H+ + HCO3-
137566
B/L acids HBr, NH4, H3O, HSO3, H20 respectively. the other reactant is a B/L base.
551403
the acids are carboxalic acid and  carbonic acid
748799
an acid is a proton donor while a base is a proton acceptor or an electron donor\n Hope i'm right
728949
They are (Listed in order of decreasing strength)\nIonic interactions \nHydrogen bonds \ndipole-dipole interactions \nLondon dispersion forces (Van der Waals force).\n\nA very approximate strength order would be: \nBond type/Relative strength \nIonic bonds/1000 \nHydrogen bonds/100 \nDipole-dipole/10 \nLondon (Van der Waals) Forces/1
711408
I am not a chemistry student but I make this research for you and maybe it helps you http://www.chem.latech.edu/~deddy/chem104/104Antacid.htm\nhttp://www.chemcool.com/regents/acidsbasessalts/aim3.htm\n\njust copy those links and you should be on your way to solve ur problem.
30128
I takes a bit of familiarity.  You need to know which ones will ionize in solution, and how they'll ionize.  Anything that releases a H ion is an acid.\n\nIf you have a specific list, I can try to help; elsewise you're best to look them up individually or study a bunch of inorganic and organic chemistry until you can spot the ionization trends.  In biochemistry, anything with the "-COOH" motif is a carboxylic acid, and is colloquially called an acid.\n\nThere's alos a tendency--though it isn't rock-solid--to write  ionizing substances in a conjugate acid/conjugate base manner.  Generally, things that have H as the first element listed will be acids (H3PO4, HCl, HBr, HI, HF, HNO3, H2SO4, HClO4, H3BO3, H2CO3, and HClO3 are all acids).  Organic acids are not necessarily going to fit into this scheme.
877634
Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+
708448
This deals with Bronsted-Lowry (B-L) acids and bases, and conjugate-base pairs \n\nB-L acids: donate H+ ions: STRONG ACIDS dissociate into ions\nH20 + HCl --> Cl- + H+  (H+ is the same as hydronium [H3O+])\nso it can be written as H20 + HCl --> Cl- + H3O+ \nThis looks like it donates a H+ ion, but it dissociates because it is a STRONG acid.  \n\nwk acid: HA= wk acid; A- = conjugate base\nHA + H2O ---> H3O+ + A-\n\nB-L bases: accept H+ ions: STRONG bases dissociate\nNaOH + H2O --> H2O + Na+ + OH-\n\nwk base: B = wk base; HB = conjugate acid\nB- + H2O --> HB + OH-\n\nThat's all you need to know to write all eqns.
739042
2Al + 6HNO3 ----> 2Al(NO3)3(s) + 3H2(g)
948423
You are going the wrong way.\nThe dissociation constant of a weak monoprotic acid is Ka. If you have a polyprotic acid then you have Ka1,Ka2,etc and more than one equivalence points.\n\nDo the plot, find the equivalence point, and then pKa=pH for 1/2 volume of base of that needed to reach the equivalence point.\nSince you have a weak acid you don't have the equivalence point at pH=7 but at higher pH (The equivalence point will be at the middle of the rising curve). \nThen Ka=10^-pKa\n\nYou can have a look at \n\nhttp://www.shodor.org/unchem/basic/ab/\n\nhttp://www.chemguide.co.uk/physical/acidbaseeqia/phcurves.html
781970
2Al + 3F2 ----> 2AlF3\nAl + 3OH- ----> Al(OH)3
297078
What are the pka's of all the different species? It sounds like the end product is a mess of conjugate bases, so the pka's are needed to figure out which disassociation reaction will predominate.
880704
The pH of the salt depends on the strengths of the original acids and bases:\n\nAcidBaseSalt pH\nstrongstrongpH = 7\nweakstrongpH > 7\nstrongweakpH < 7\nweakweakdepends on which is stronger\n\nThat should be what you want.
744922
HClO2 + Ba(OH)2 -> BaClO2 + H2O\n\n2(NH4)3PO4 + 3Ca(NO3)2 -> 6(NH4)(NO3) + Ca3(PO4)2\n\nFinished and balanced.
899424
2 M HCl\n\nHCl is a strong acid and acids have pH less than 7\n\nH3PO4 is a weak acid\n\nNH3 is a base\n\nNaOH is a base