Calculate the [H+] in each of the following solutions and
indicate whether the solution is acidic...
Calculate the [H+] in each of the following solutions and
indicate whether the solution is acidic or basic? a) [OH-] = 2.32 X
10^-4 M b)[OH-] = 8.99 x 10^-10 M c) [OH-] = 4.34 x 10^-6 M d)
[OH-] = 6.22 x 10^-12 M
16.29 calculate [H+] for each of the following solution and
indicate whether the solution is acidic, basic, or neutral.(b)
[OH-]= 8.8 * 10-9 M; (c) a solution in which [OH-] is 100 times
greater than [H+] SHOW ALL WORK
(ASAP) Indicate whether each of the following compounds will
gave an acidic, basic or neutral solution when dissolved in water.
Clear All ammonium bromide calcium fluoride potassium perchlorate
potassium bromide The pH will be less than 7. The pH will be
approximately equal to 7. The pH will be greater than 7.
ammonium
bromide
calcium
fluoride
potassium
perchlorate
potassium
bromide
Indicate whether each of the following compounds will gave an
acidic, basic or neutral solution when dissolved in water.
Clear All
ammonium bromide
barium cyanide
potassium chloride
potassium bromide
The pH will be less than 7.
The pH will be approximately equal to 7.
The pH will be greater than 7.
Consider 0.25 M solutions of the following salts. For each salt,
indicate whether the solution is acidic, basic, or neutral.
basic neutral acidic CsF
basic neutral acidic NaCl
basic neutral
acidic C2H5NH3NO3
basic neutral
acidic H2NNH3Cl
basic neutral acidic CsNO3
basic neutral acidic RbOCl
Predict whether the following salt solutions are neutral,
acidic, or basic, and calculate the pH of each. Hint: Write the
equation for dissociation of the salt and any equilibrium
established.
0.25 M NH4Br; KB of NH3 = 1.8×10−5 0.10 M NaCN;
KA of HCN = 4.9×10−10 0.20 M NaNO2;
KA of HNO2 = 4.6×10−4
State whether 0.1 M solutions of each of the following salts are
acidic, basic, or neutral. explain your reasoning for each by
writing a balanced net ionic equation to describe the behavior of
each non-neutral salt in water: NaCN, KNO3, NH4Cl, NaHCO3, and
Na3PO4
Identify the single most acidic or basic principle species in
each of the following solutions. Calculate its molarity or number
of moles (your choice). In the case of any species other than H3O+
or OH-, write the net ionic equation for the reaction of that
speicies with water. Calculate the pH of each solution.
a) 10.0 mL of 0.30 M HCL
b) 10.0 mL of 0.35 M HF
c) 10.0 mL of 0.25 KOH
d) 15.0 mL of 0.30 M...
Indicate if the aqueous solutions of the following salts would be
acidic, basic, neutral, or “need more information”.
LiNO3
(C5H5NH)(CH3COO)
LiOCN
(CH3NH3)Cl
RbClO4
NH4I
Indicate if the aqueous solutions of the following salts would be
acidic, basic, neutral, or “need more information”.
LiNO3
(C5H5NH)(CH3COO)
LiOCN
(CH3NH3)Cl
RbClO4
NH4I
calculate the [H+] and the pH of each of the
solutions. {Show calculation for a, c, d, e, h, j, and k.}
a) 0.358 M HNO3 pH =
:[H+]
=
e) 0.358 M HF pH =
:[H+]
=
i) 0.358 M HC6H5O pH =
:[H+]
=
b) 55.5 M H2O pH =
:[H+]
=
f) 0.358 M HNO2 pH =
:[H+]
=
j) 0.358 M Ba(OH)2 pH =
:[H+]
=
c) 0.358 M NaOH pH =
:[H+]
=
g) 0.358 M
CH3NH2 pH =...