If the salt formed is KCl what is the parent acid and the parent base?
489210
Potassium Hydroxide and Hydrochloric acid.\n\nKOH + HCl = KCl + H2O
828596
It reacts when in contact with any acid material. When combined with an acid, it forms a salt.
1154298
A salt is formed between the reaction of an acid and a base. Usually, a neutral salt is formed when a strong acid and a strong base is neutralized in the reaction: \n           H+ + OH- = H2O \nThe bystander ions in an acid-base reaction form a salt solution. Most neutral salts consist of\ncations: Na+,K+,Rb+,Cs+,Mg2+,Ca2+,Sr2+,Ba2+ \nanions:  Cl-,Br- ,I-,ClO4-,BrO4-,ClO3-,NO3-\nThese ions have little tendency to react with water. Thus, salts consisting of these ions are neutral salts. For example: NaCl, KNO3, CaBr2, CsClO4 are neutral salts.\n \nWhen weak acids and bases react, the relative strength of the conjugated acid-base pair in the salt determines the pH of its solutions. The salt, or its solution, so formed can be acidic, neutral or basic. A salt formed between a strong acid and a weak base is an acid salt, for example NH4Cl. A salt formed between a weak acid and a strong base is a basic salt, for example NaCH3COO. These salts are acidic or basic due to their acidic or basic ions.\nAcidic ions: NH4+,Al3+,Pb2+,Sn2+.\nTransition metal ions: HSO4-, H2PO4- \nBasic Ions: F-,C2H3O2-,NO2-,HCO3-,CN-,CO32-,S2-                 SO42-,HPO42-,PO43-
300034
Potassium chloride occurs as either white, granular powder or as colorless, elongated, prismatic or cubical crystals. It is odorless and has a saline taste. One gram of potassium chloride contains 13.4 mEq of potassium. Potassium chloride may also be known as KCl.\n\n \n\nPotassium gluconate occurs as white to yellowish white, crystalline powder or granules. It is odorless and has a slightly bitter taste and is freely soluble in water. One gram of potassium gluconate contains 4.3 mEq of potassium.
788070
Well its easy dear.\n\n2Li (s) + Cl2 (g) ----> 2 LiCl (s)
167726
potassium can form many compounds. such as KCN KCl KOH et cetera.
200802
1. acid\n2. salt\n3. no idea\n4. salt\n5. base\n6. no idea\n7. salt\n8. base\n9. salt\n10. acid\n11. base
378003
pH for a salt of strong base and weak acid is given by:\n         pH = 7 - (1/2)pKb - (1/2)log C\nwhere pKb = dissociation const of strong base\n       C  = concentration of Acid.\n\nKb = Kw / Ka = (10^-14) / (6.5 x 10^-5) = 1.53x10^-10\npKb = -log (1.53x10^-10) = 9.8154\nlog C = log 10^-1 = -1\n\npH = 7 - (1/2)x 9.8154 - (1/2)x-1\n   = 7 - 4.9077 + 0.5\n   = 2.5923
588293
When an acid reacts with an alkali (base), neutralisation occurs as the pH of the mixture becomes neutral, pH=7. (Acidic: pH < 7, Basic: pH > 7).\n\nSo an example would be to react sulphuric acid with sodium hydroxide to form sodium sulphate (salt) and water.\n2NaOH + H2SO4 ---> Na2SO4 + 2H20\n\nAn ELEMENT that would neutralise sulphuric acid (i.e. make its pH 7) could be any metal.\n\ne.g. Mg + H2SO4 ---> MgSO4 + H2\n\nBut this is not called a neutralisation reaction.
1179756
Always remember that salts are formed by ions:\n\nCommon salt-forming cations include:\n\nammonium NH4+ \ncalcium Ca2+ \niron Fe2+ and Fe 3+ \nmagnesium Mg2+ \npotassium K+ \npyridinium C5H5NH+ \nquaternary ammonium NR4+ \nsodium Na+\n\nCommon salt-forming anions (and the name of the parent acids in parentheses) include:\n\nacetate CH3COO− (acetic acid) \ncarbonate CO32− (carbonic acid) \nchloride Cl− (hydrochloric acid) \ncitrate HOC(COO−)(CH2COO−)2 (citric acid) \ncyanide C≡N− (hydrogen cyanide) \nhydroxide OH− (water) \nnitrate NO3− (nitric acid) \nnitrite NO2− (nitrous acid) \noxide O2− (water) \nphosphate PO43− (phosphoric acid) \nsulfate SO42− (sulfuric acid)
91741
What are the states of each of the substances?\n\n\nammonium chloride(aq)+potassium hydroxide(aq)---->ammonium hydroxide(aq)+potassium chloride(aq)\n\n   Complete ionic equation\nNH4+(aq)+Cl-(aq)+K+(aq)+OH-(aq)------->\nNH4+(aq)+OH-(aq)+K+(aq)+Cl-(aq)\n\n     Net Ionic Equation\nSame as complete ionic equation, every ion is a spectator ion, OR it doesn't exist.\n\nI don't think both substances are in aqueous solution.
706351
KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
356281
MgCO3 + 2HCl ---> MgCl2 + CO2 + H2O\n\n2HCl + MgO ---> H2O + MgCl2\n\nBarium hydroxide is a base so can be neutralised with any acid.  An example being HCl.\n\nBa(OH)2 + 2HCl ---> BaCl2 + 2H2O\n\nor H2SO4\n\nBa(OH)2 + H2SO4 ---> BaSO4 + 2H2O
160963
K2SO4 ---> 2K+  +  SO4-\n\nHCl ---> H+  +  Cl-\n\nNaHCO3 ---> Na+  +  HCO3-\n\nNH4OH ---> NH4+  +  OH-\n\nBaCl2 ---> Ba-2  +  2CL-\n\n(NH4)3PO4 ---> 3NH4+  +  PO4-3
192443
Write down the equation of reaction: K + Cl2 -> KCl (not balanced)\n\nBalance the equation of reaction: 2K + Cl2 -> 2KCl (balanced)\n\nFind the moles of Potassium: 5 g K / 39.10 g/mol K = 0.128 mol\n\nFind the moles of Chlorine gas: 7 g Cl2 / (2 x 35.45 g/mol) = 0.098 mol\n\nDetermine the stoichiometric ratios: \nCl2 -> 2 KCl\nK ->   KCl   \n\nFind the moles of product: \n\nFor potassium: 0.128 mol K x (1 mol KCl / 1 mol K) = 0.128 mol KCl\n\nFor chlorine:  0.098 mol Cl2 x (2 mol KCl / 1 mol Cl2) = 0.196 mol KCl\n\nSo potassium is the limiting reactant. \n\nMass of KCl that can be formed: 0.128 mol K x (1 mol KCl / 1 mol K) x (39.10 g/mol K +  35.45 g/mol Cl) =  9.54 g KCl
662629
Wrrite the balanced eqution.  The acid and base will react to give water and the salt.  There will be so much acid left.  Calculate the pH of that amount of acid with the salt formed present.  THis is a buffer calculation.
991396
A potassium ion has one positive charge because it is missing one valence electron.   So K can form compounds with anything that is electronegative; in other words, any atom or molecule that likes to grab electrons. Anything at the right hand end of the periodic table, like O, S or the halogens for instance.   Or a more complicated compound would be with an organic acid like stearic acid; you replace one H with a K and you get a liquid soap.   If you used Na instead of K you'd get the usual solid soap.   When I was a kid in Britain, the soap in public bogs was liquid so you couldn't steal it.