Rank the following 0.10 M solutions in order of increasing pH.
(c) LiOH, LiClO4, HONH3ClO4, LiOBr, HClO4, HOBr, HONH2
HClO4< HOBr<HONH3ClO4<LiClO4<LiOBr<HONH2<LiOH
HCLO4 is a very strong acid.
strong acids have weak conjugate bases.
Metal Hydroxides are strong bases .
pH increases with basicity and decreases with acidity.
Hence the order.
Rank the following 0.10 M solutions in order of increasing pH. (c) LiOH, LiClO4, HONH3ClO4, LiOBr, HClO4,...
Rank the following 0.10 M solutions in order of increasing pH. (Use the appropriate <, =, or > symbol to separate substances in the list.) a) RbClO4, HONH2, HClO4, RbOH, HONH3ClO4, RbOBr, HOBr
Rank the following 0.10 M solutions in order of increasing pH. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) RbF, RbBr, HBr, HF (b) LiI, NH4I, HI, NH3 (c) RbOH, RbOBr, HONH3ClO4, HOBr, HClO4, HONH2, RbClO4
Assuming each solution to be 0.10 M , rank the following aqueous solutions in order of decreasing pH. Rank the solutions from the highest to lowest pH. To rank items as equivalent, overlap them N2H2 Ba(OH)2 HOCL NAOH HCL
12.59 Place the following solutions in order of increasing [H3O+]. Please explain your reasoning. 0.10 M HF, 0.10 M NH3, 0.10 M HNO3 0.10 M HCN, 0.20 M HCN, 0.20 M HClO4 0.10 M NH3, 0.10 M NaOH, 0.10 M Ca(OH)2
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...
Assuming equal concentrations, rank these solutions by pH. Highest pH to Lowest pH. HClO4(aq) Sr(OH)2(aq) NH3(aq) KOH(aq) HF(aq)
Assuming equal concentrations, rank these solutions by pH. CaBr2 LiOH CH3NH3Br HClO4 Mg(ClO)2
Calculate the pH of each of the following strong acid solutions. (a) 0.00438 M HClO4 pH = (b) 0.579 g of HCl in 21.0 L of solution pH = (c) 59.0 mL of 3.90 M HClO4 diluted to 4.50 L pH = (d) a mixture formed by adding 69.0 mL of 0.00809 M HClO4 to 78.0 mL of 0.00483 M HCl pH =
Calculate the pH of each of the following strong acid solutions. (a) 0.00471 M HClO4 pH = (b) 0.329 g of HBr in 16.0 L of solution pH = (c) 65.0 mL of 7.50 M HClO4 diluted to 4.60 L pH = (d) a mixture formed by adding 54.0 mL of 0.00155 M HClO4 to 47.0 mL of 0.00191 M HBr pH =
A 900.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH at 25 degree C. Determine the pH of the solution after the addition of 600.0 mL of LiOH.