Q: How many grams of NaNO, is needed to prepare an aqueous solution of 170 mL with a pH of 8.54? (For…
A: Consider the initial concentration of NO2- to be C and the reaction can be depicted as; Here, x=…
Q: what is the pH of 1.0 x 108 M solution of H2S04? Ka for the reaction is100 Select one: О а. 8.00 ОБ.…
A: In order to calculate the pH we first write down the given data: Concentration of the acid= 10-8 M.…
Q: What is [H] in a 0.430 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 × 10 5)? %3D
A:
Q: What is the pH of a 0.40 M ammonia solution? Ka is 5.6 X 10-10 11.43 O 2.57 O 9.18 O 4.82
A: Ka = 5.6 x 10 —10
Q: All of the following are examples of hard bases EXCEPT: O Co,2- OH H20 SH
A: Hard base: Electron pair donor atom is not easily polarizable like N, O, F. Soft base: Electron pair…
Q: What is the pH of a 0.200 M solution of HNO3? A 0.70 B 1.31 c) 6.18 (D) 8.53
A: Given, the concentration of HNO3 =0.200 Mwe are asked to calculate the pH of solution of HNO3
Q: What is the pH of .08 M H2SO3 (aq)? O 12.51 Ο 1.10 0 .94 O 1.89 Ο 1.49
A: Concentration of H2SO3 = 0.08 M pH of the H2SO3 = ?
Q: A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC gH 70 4) was dissolved in enough…
A:
Q: Calculate the pH of a 0.043 M NaF solution. (K, for HF = 7.1 x 104.)
A: Given -> Molarity of NaF = 0.043 M Ka ( HF) = 7.1 × 10^ -4
Q: The pH of a solution for which [OH-] = 1.0 x10-6 is %3D
A: pH stands for Hydrogen potentials. pH is a negative logarithm of the concentration of hydrogen ions.…
Q: What is the pH of a 0.25 M solution of NH3? Kb = 1.8x105 O 2.67 O 11.33 O 9.07 O 4.93
A: Given valuues from the question, Salt concentration = c= 0.25 M Kb =1.8×10--5 then,
Q: What is the pH of a 0.100 M solution of LiBrO(aq) at 25'C? Assume that LiBrO is a strong…
A: Since you have posted multiple questions, we are entitled to answer the first only. Given:…
Q: The pOH of a 0.025 M of HCIO4 is O a. 12.40 ОБ. 0.94 O c. 13.06 O d. 1.60
A:
Q: What is the percent ionization at 25 °C for a 0.00675 M solution of codeine (CH2, NO)? O 18.7% O…
A:
Q: Calculate the pH of a 0.20 M solution of NaC2H302. HC2H302 has a Ka=1.8 x 10. O a. 7.00 O b. 4.98 O…
A: i would go for option b- 4.98 as acid concentration is missing so i am unable to give you a solution…
Q: A solution of CSH5N (pyridine, Kp = 1.7 x 10 °) has a pH of 9.40. What is the [C5H5N]? O 9.3 x 1011…
A:
Q: What is the pH of a solution with [H*] = 1.0 x 104 M? 0 7 O -4 O 4 O 10
A: The pH of the solution is defined as negative logarithm of the molar concentration of H+ ions.…
Q: What is the pOH of a 0.053 M solution of KOH at 25 °C? 1.28 12.72 13.11 0.89
A: We have given for KOH solution. Concentration of KOH solution = 0.053 M KOH will dissociates as;…
Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93
A:
Q: What is the pH of a 0.193 M w. acid HA solution? Ka = 6.61 x 10−6?
A: The acid is weak so it weakly dissociates in the solution. That is it gives an H+ ions slowly in to…
Q: The pH of 0.20 M HNO3 is O a. 0.63 O b. 1.58 O C. 0.70 O d. 0.20
A: pH = - log [H+ ] Strong acids undergo complete ionisation in solution. Thus, [H+] =…
Q: calculate the ph of a 0.600 solution of Na2S
A: When Na2S dissolved in water - Na2S + 2H2O <===> 2NaOH + H2S Thus, sodium Sulfide is a salt of…
Q: What is the pH of 7.8 x 105 M HNO3 (aq)? O 18.1 O 9.9 O 9.5 O 3.7 O 4.1
A:
Q: Calculate the pH and [S2−] in a 0.10-M H2S solution. Assume ka1= 1.0 × 10−7; ka2= 1.0 × 10−19.
A: Answer:- This question is answered by using the simple concept of calculation of pH of a weak acid…
Q: What is the pH of a 0.20 M solution of CH3NH3NO3 at 25 °C? At this temperature, the Kp for CH3NH2 is…
A: Both given Ka and Kb are given, means this salt is a weak acid-weak base type salt. -PH or [H+] of…
Q: For a 1.0 x 10-6 M solution of HNO3(aq) at 25 °C, arrange the species by their relative molar…
A:
Q: What is the pH of a 9.27*105 M solution of H3O? O 4.03 O 9.97 O 12.81 O 2.98
A: (10) Kool aid a powdered substance when added with water or solvent, will give a flavored sugary…
Q: : What is the pH of a 0.400 M HNO O 0.40 O 2.05 O 0.60 O 4.12 O 1.67
A: HNO3 when dissolved in water it dissociates.
Q: A 1.2 · 102 M aqueous solution of Ca(OH)2 at 25.0 °C has a pH of, O 12.38 O 12.08 O 1.62 O 2.4 · 102…
A:
Q: Which of the following statements is true about an aqueous solution of NH,CN? K, (HCN) - 4.9 x 10…
A: Since you have posted multiple questions, we are entitled to answer the first only.
Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.
A: Concentration of Al ion = 0.064 M
Q: If [H3O*] = 3.8 x 10-3 M, what is the pOH of the solution? %3D O 2.42 O 2.13 O 2.77 11.58
A: The given data contains, H3O+=3.8×10-3M.
Q: Calculate the pH of a of 0.100M KBRO solution. Ka for hypobromous acid, HBRO, is 2.0 x 10 6- 10.85…
A: Given: The concentration of the KBrO3 solution = 0.100 M The Ka for HBrO3 = 2.0 × 10-9 We have to…
Q: Which of the following is a BrØnsted-Lowry acid? O C Cl 4 Ο ΝΗ O PH, Ο ΝΗ5 O Br 2
A:
Q: Calculate the pH of a solution resulting from the addition of 50.0 mL of 0.30M HNO3 to 50.0 mL of…
A: Nitric acid which is a strong acid on undergoing a reaction with ammonia will form a salt of…
Q: What is the percent ionization of an 3.5 M HF solution? (Ka=6.6 x 104) O 1.4 % O 0.22 % O2.4 % O 1.7…
A:
Q: What is the pH of a 0.0670 M solution of methylamine (CH3NH2, Kb = 4.4 x 104)? %3D
A:
Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 × 10-5) O 4.94 O 12.03 O 1 1.05 O 8.02 O 2.09
A: Given, Concentration of NH3 = [NH3] = 0.075 M Base dissociation constant of NH3 = Kb = 1.75 x 10-5…
Q: What is the pH of a 0.1055 M CH3COOH solution (K, = 1.75 x 10-5)? %3D
A: Answer: ICE table for the dissociation of weak monoprotic acid is shown below:
Q: What is the pH of a solution with [H3O+] of 1.9 x 10-8 M?
A: Given that, [H3O+] = 1.9×10-8 M pH = ?
Q: .Calculate the concentration of H3O+ in the sample of milk of magnesia with the pH=10.52 2.…
A: “Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: Calculate pH of a solution containing 0.50 M NaOCI and 0.75 M HOCI. (K, of HOCI = 3.2 x 10 8) O7.89…
A:
Q: Calculate the pH of a 0.50 M solution of ammonia (NH3, Kb = 1.8 x 10P.) A. 9.22 B. 2.52 C. 9.26 D.…
A: It is known that ammonia is a weak base in its aqueous solutions. The dissociation reaction in the…
Q: Question attached
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Q: Calculate the pH of a 3.5 x 10-3 M HNO3 solutio O 2.46 O 3.46 O 0.54
A: The acidity of the solution is measured by the pH scale. pH scale ranges from value 1 to 14. The…
Q: The K, for hypoiodite anion (IO) is 4.35x10-4. What is the pH of a 0.226 mol L solution of lithium…
A:
Q: The pOH of a 0.025 M of HCIO4 is O a. 12.40 O b. 0.94 O c. 13.06 O d. 1.60
A: According to Arrhenius acid base theory, an acid is a substance which can give up proton(H+) to…
Q: What is the pH of a solution with [H3O+] = 4.5 x 10-5M?
A:
Q: What is the pH of a 0.35 M solution of methylamine (CH3NH2, Kb 4.4 at 25°C? O a. 5.55 b. 12.09 O c.…
A: We will. Calculate pH
Q: Calculate the pH of water containing 0.05 M NaCl at 25°C. Given: YH = 0.86 and %3D YOH- = 0.81. O…
A:
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- What is the pH at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s law constant forCO2 at 25 °C is 3.1 x 10-2 mol/L-atm.A solution of volume 0.500 L contains 1.68 g NH3 (Kb = 1.8 x 10^-5) and 4.05 g (NH4)2SO4. What is the pH of this solution?Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5.
- If a 0.55 M solution of a monobasic compound B has a pH of 11.32, what is the Kb value of the base B?What is the degree of ionization (i) for H₂SO₄(aq)?The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of H2CO3/HCO3− is required to obtain a pH of 7.40, the pH of blood? (Assume that the Ka of H2CO3 is 4.4 ✕ 10−8.)
- The pH of a solution of 0.63 M pyridine is 9.51, what is the Kb of pyridine? What is the Ka of its conjugate acid?For a 1.0×10−6 M1.0×10−6 M solution of HNO3(aq)HNO3(aq) at 25 °C,25 °C, arrange the species by their relative molar amounts in solution. NO^-3, HNO3, OH^-, H2O, H3O^+Rain with a pH below 5.6 is considered acid rain. The principal cause of acid rain is coal-burning electrical power plants (sulfurous and sulfuric acids are formed in the atmosphere from this). Any combustion reaction that produces high temperature can also produce acid rain (nitrous and nitric acid are produced in the atmosphere from this). Thus, automotive engines are also an important contributor to acid rain. Acid rain harms both living and nonliving things in a variety of ways. What solution/s can you propose to combat acid rain?